Search found 101 matches
- Sun Mar 14, 2021 10:50 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Saying Thank You to Dr. Lavelle
- Replies: 490
- Views: 513211
Re: Saying Thank You to Dr. Lavelle
Dear Dr. Lavelle, As a UCLA student, I am happy and proud to say that you were my first chemistry instructor at the college level. While I had some experience with AP Chemistry in high school, you made my experience wonderful and truly remarkable! You made learning chemistry for myself, and as I am ...
- Mon Mar 08, 2021 7:53 am
- Forum: Kinetics vs. Thermodynamics Controlling a Reaction
- Topic: Slow Step
- Replies: 21
- Views: 791
Re: Slow Step
Hi,
Yes! The slow step will be assumed to have the higher activation energy, while the faster step will have the lower activation energy. There is no threshold number, it it just based on comparison.
Hope this helps! :)
Yes! The slow step will be assumed to have the higher activation energy, while the faster step will have the lower activation energy. There is no threshold number, it it just based on comparison.
Hope this helps! :)
- Mon Mar 08, 2021 7:52 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: What is the purpose of having a salt bridge?
- Replies: 16
- Views: 674
Re: What is the purpose of having a salt bridge?
Hi, Before we can understand why we need a salt bridge, we need to first understand what happens to a galvanic cell without one. Without one, we know that electrons would simply migrate from the anode to cathode. However, there is no counteractive force to prevent the electrons from accumulating or ...
- Mon Mar 08, 2021 7:48 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: K
- Replies: 33
- Views: 1242
Re: K
Hi,
K_c is typically referred to the equilibrium constant in terms of concentrations. However, K is a more general form of the equilibrium constant that may be adapted to multiple situations (such as K_p in terms of partial pressures).
Hope this helps! :)
K_c is typically referred to the equilibrium constant in terms of concentrations. However, K is a more general form of the equilibrium constant that may be adapted to multiple situations (such as K_p in terms of partial pressures).
Hope this helps! :)
- Mon Mar 08, 2021 7:47 am
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: n in ∆G = -nFE
- Replies: 80
- Views: 3804
Re: n in ∆G = -nFE
Hi, Whenever we are balancing half reactions into an overall reaction, you must balance the electrons on both sides to ensure they cancel out. That number of electrons will be considered "n." For example, assume you have a redox reaction where there are 3 e- on the left and 2 e- on the rig...
- Mon Mar 08, 2021 7:44 am
- Forum: General Rate Laws
- Topic: Rate determining step
- Replies: 38
- Views: 1408
Re: Rate determining step
Hi, The slow step is the rate determining step because it dictates how fast the reaction can go overall. For instance, if we assume the initial rates of Step 1 and Step 3 are 50 M/s and 60 M/s respectively, yet Step 2 is proceeding at 20 M/s the reaction cannot go faster than 20 M/s because the slow...
- Mon Mar 01, 2021 7:52 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Anodes and Cathodes
- Replies: 22
- Views: 962
Re: Anodes and Cathodes
Hi,
At the anode oxidation occurs, while in the cathode reduction occurs.
Hope this helps! :)
At the anode oxidation occurs, while in the cathode reduction occurs.
Hope this helps! :)
- Mon Mar 01, 2021 7:50 am
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: Max cell potential
- Replies: 4
- Views: 285
Re: Max cell potential
Hi,
You can think of a system having the maximum cell potential at the very instant the cell is formed where the current is just on the verge of forming between the anode and the cathode.
Hope this helps! :)
You can think of a system having the maximum cell potential at the very instant the cell is formed where the current is just on the verge of forming between the anode and the cathode.
Hope this helps! :)
- Mon Mar 01, 2021 7:48 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Salt bridge
- Replies: 10
- Views: 533
Re: Salt bridge
Hi, The purpose of a salt bridge is to prevent a build up of charge. A good analogy I can think of is where the wire connecting the two cells is a road with the electrons as the cars. If too much traffic is on one side, then the cars can no longer move to the other side to do electrical work. Now, r...
- Mon Mar 01, 2021 7:44 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Oxidation potentials Textbook Problems
- Replies: 2
- Views: 200
Re: Oxidation potentials Textbook Problems
Hi,
I believe the book assumes you are using the Appendix in order to solve these type of problems.
Thus, on the exam if you were given a problem similar I think you would be given the corresponding E values.
Hope this helps! :)
I believe the book assumes you are using the Appendix in order to solve these type of problems.
Thus, on the exam if you were given a problem similar I think you would be given the corresponding E values.
Hope this helps! :)
- Mon Mar 01, 2021 7:41 am
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: n in ∆G = -nFE
- Replies: 80
- Views: 3804
Re: n in ∆G = -nFE
Hi, n refers to the moles of ELECTRONS transferred in a redox reaction. In order to find this amount, you would need to split the overall reaction into two half reactions (oxidation and reduction) and then balance them accordingly. However, when you're balancing you need to ensure the number of elec...
- Mon Feb 22, 2021 7:55 am
- Forum: Van't Hoff Equation
- Topic: Celcius vs Kelvin for T1 and T2
- Replies: 84
- Views: 6440
Re: Celcius vs Kelvin for T1 and T2
Hi, A good rule of thumb is always use Kelvin for your thermodynamic equations. In MOST (not all) cases, we have to use Kelvins because the constants we are given (such as the ideal gas constant) are expressed in terms of Kelvin (this ensures it cancels out for your final answer). Hope this helps! :)
- Mon Feb 22, 2021 7:53 am
- Forum: Balancing Redox Reactions
- Topic: Oxidizing vs Reducing
- Replies: 55
- Views: 2249
Re: Oxidizing vs Reducing
Hi, A good rule of thumb is to always first find out what undergoes oxidation and what undergoes reduction. Then, in order to identify the corresponding agent, it would be the opposite. For example, assume in a hypothetical reaction nitrogen (N) is oxidized from 0 to 4+. Therefore, nitrogen would be...
- Mon Feb 22, 2021 7:50 am
- Forum: Balancing Redox Reactions
- Topic: "Leo" Oxidation Numbers
- Replies: 26
- Views: 1059
Re: "Leo" Oxidation Numbers
Hi,
The acronym "LEO" means "loss of electrons = oxidation."
This is just a house keeping rule we have to remember what we mean when something is oxidized.
Hope this helps! :)
The acronym "LEO" means "loss of electrons = oxidation."
This is just a house keeping rule we have to remember what we mean when something is oxidized.
Hope this helps! :)
- Mon Feb 22, 2021 7:49 am
- Forum: Calculating Standard Reaction Entropies (e.g. , Using Standard Molar Entropies)
- Topic: Molar Entropy
- Replies: 10
- Views: 1036
Re: Molar Entropy
Hi, As previously said, for molar entropy we always tend to look for molecules which are more complex (i.e. those which are more disordered under similar conditions relative to whatever we are comparing). If we are comparing elements, we would look at atomic number as the inclusion of more protons (...
- Mon Feb 22, 2021 7:46 am
- Forum: Balancing Redox Reactions
- Topic: Oxygen
- Replies: 12
- Views: 620
Re: Oxygen
Hi,
Typically, we would see that oxygen (O2) would have an oxidation number of 0 as it is in their elemental form.
Hope this helps! :)
Typically, we would see that oxygen (O2) would have an oxidation number of 0 as it is in their elemental form.
Hope this helps! :)
- Mon Feb 15, 2021 7:53 pm
- Forum: Calculating Work of Expansion
- Topic: Irreversible vs reversible
- Replies: 5
- Views: 302
Re: Irreversible vs reversible
Hi, If an expansion is considered irreversible, you think of it as a rapid expansion. In other words, it happens so fast that you can't go back to your initial condition. If an expansion is considered reversible, you can think of it as a slower expansion. In other words, because it is happening in i...
- Mon Feb 15, 2021 7:50 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: confusion on using Cp and Cv
- Replies: 24
- Views: 1023
Re: confusion on using Cp and Cv
Hi, Yes! Recall, C refers to the heat capacity, or the amount of heat to raise the temperature of a substance by 1 unit of temperature. The subscript "P" or "V" is indicative of what variable we are assuming is constant. If it is "C_p," then it is the heat capacity at c...
- Mon Feb 15, 2021 7:48 pm
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: Isothermal Reactions
- Replies: 26
- Views: 1168
Re: Isothermal Reactions
Hi,
Yes! When we discuss isothermal reactions, we assume they are reversible reactions in equilibrium where the external and internal pressure of the system is the same. Also, there is no temperature change (iso- meaning same and -thermal referring to temperature).
Hope this helps! :)
Yes! When we discuss isothermal reactions, we assume they are reversible reactions in equilibrium where the external and internal pressure of the system is the same. Also, there is no temperature change (iso- meaning same and -thermal referring to temperature).
Hope this helps! :)
- Mon Feb 15, 2021 7:46 pm
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: Which R to use
- Replies: 42
- Views: 2862
Re: Which R to use
Hi,
In order to ensure you have the proper units for entropy, you should use R = 8.314 as it has the joules (J) unit in it.
Hope this helps! :)
In order to ensure you have the proper units for entropy, you should use R = 8.314 as it has the joules (J) unit in it.
Hope this helps! :)
- Mon Feb 15, 2021 7:45 pm
- Forum: Phase Changes & Related Calculations
- Topic: Define Phase Change
- Replies: 78
- Views: 4907
Re: Define Phase Change
Hi, A phase change is defined as any transition from one of three states of matter covered in the course (solid, liquid, gas). For instance, a block of ice (solid) melting in water (liquid) is a phase change. Water vapor (gas) condensing into water (liquid) is also a phase change. Hope this helps! :)
- Mon Feb 08, 2021 9:02 am
- Forum: Calculating Standard Reaction Entropies (e.g. , Using Standard Molar Entropies)
- Topic: Spontaneous
- Replies: 20
- Views: 1172
Re: Spontaneous
Hi,
A reaction is considered spontaneous if Delta G is negative. A nonspontaneous process is where Delta G is positive.
Hope this helps! :)
A reaction is considered spontaneous if Delta G is negative. A nonspontaneous process is where Delta G is positive.
Hope this helps! :)
- Mon Feb 08, 2021 9:00 am
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: Entropy Concept
- Replies: 5
- Views: 246
Re: Entropy Concept
Hi, Entropy is a measure of disorder in a system. For instance, you could conceptually understand this with comparing a clean dorm room to a messy dorm room. In the clean room, the room is fairly organized with where everything should be, so the entropy is fairly low. In the messy room, clothes may ...
- Mon Feb 08, 2021 8:57 am
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: DeltaE vs DeltaU
- Replies: 13
- Views: 546
Re: DeltaE vs DeltaU
Hi,
I believe according to the textbook, Delta E and Delta U are both used interchangeably for the change in internal energy.
Hope this helps! :)
I believe according to the textbook, Delta E and Delta U are both used interchangeably for the change in internal energy.
Hope this helps! :)
- Mon Feb 08, 2021 8:57 am
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Using R in thermodynamic equations
- Replies: 24
- Views: 972
Re: Using R in thermodynamic equations
Hi, A good rule-of-thumb I have always used for these calculations is to not memorize which one to use, but to look at the units. For each problem, I always write down the units for everything I am given and see what cancels out. After that, I then choose which R to use depending if I have pressures...
- Mon Feb 08, 2021 8:54 am
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Does phase matter in Hess's Law?
- Replies: 21
- Views: 1848
Re: Does phase matter in Hess's Law?
Hi, Yes, it does! You always have to make sure one portion of the chemical equation is equivalent to the other side if you were to combine two equations into an overall equation (i.e. He(g) on the left and right side for an arbitrary reaction). However, if you had He(s) on the left side and He(g) on...
- Mon Feb 01, 2021 12:28 pm
- Forum: Calculating Work of Expansion
- Topic: Gas Constant
- Replies: 13
- Views: 791
Re: Gas Constant
Hi, A good rule of thumb to keep in mind is to consider the equations you are using, what units you are presented with, and what units you want in the end. For instance, if you were to solve for the pressure (P) of an ideal gas with V, n, and T known, you would have to use R = 0.08206 L atm K- mol-,...
- Mon Feb 01, 2021 12:24 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: R Constant
- Replies: 91
- Views: 5214
Re: R Constant
Hi, Yes. BUT! As a bookkeeping rule it is always useful to look at what units you have presented in front of you along with the units the problem is asking you to solve for. This way, you'll be able to make sure the proper units cancel out to get what you want, whether you want atm or J. Hope this h...
- Mon Feb 01, 2021 12:22 pm
- Forum: Phase Changes & Related Calculations
- Topic: endothermic/exothermic
- Replies: 43
- Views: 4328
Re: endothermic/exothermic
Hi, Instead of memorizing the signs, it would be useful to understand what is going on at the particle level. As we go from solid to liquid to gas, the particles are allowed higher motility and are separated at farther distances from each other. Now, this would not normally happen on its own to the ...
- Mon Feb 01, 2021 12:19 pm
- Forum: Calculating Work of Expansion
- Topic: What is V1 and V2
- Replies: 12
- Views: 669
Re: What is V1 and V2
Hi,
V1 would be considered as the initial volume (V_i) and V2 would be considered the final volume (V_f).
Hope this helps! :)
V1 would be considered as the initial volume (V_i) and V2 would be considered the final volume (V_f).
Hope this helps! :)
- Mon Feb 01, 2021 12:18 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Hess's Law
- Replies: 58
- Views: 2790
Re: Hess's Law
Hi, Hess's Law may be thought of as a principle where, because the enthalpies of reactions are state functions (i.e. path doesn't matter), we may alter them accordingly to figure out the enthalpy of other reactions we may not know. For instance, we can reverse a reaction (flip to sign of delta H) or...
- Mon Jan 25, 2021 10:22 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Acid and Bases
- Replies: 7
- Views: 365
Re: Acid and Bases
Hi,
Recall, the conjugate seesaw is a good determinant of the magnitude of [H+] in comparison to [OH-].
If the solution is acidic overall, then [H+] > [OH-].
If the solution is basic overall, then [H+] < [OH-}.
If the solution is neutral overall, then [H+] = [OH-].
Hope this helps! :)
Recall, the conjugate seesaw is a good determinant of the magnitude of [H+] in comparison to [OH-].
If the solution is acidic overall, then [H+] > [OH-].
If the solution is basic overall, then [H+] < [OH-}.
If the solution is neutral overall, then [H+] = [OH-].
Hope this helps! :)
- Mon Jan 25, 2021 10:20 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Water
- Replies: 7
- Views: 341
Re: Water
Hi,
It means water can either donate a proton (acts as an acid) or it can accept a proton (acts as a base).
Hope this helps! :)
It means water can either donate a proton (acts as an acid) or it can accept a proton (acts as a base).
Hope this helps! :)
- Mon Jan 25, 2021 10:19 am
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Enthalpy changes
- Replies: 6
- Views: 282
Re: Enthalpy changes
Hi,
It would be an endothermic reaction because recall enthalpy is a state function, where the overall change in independent of the path.
Thus, if the products are above the reactants in terms of enthalpy on an energy profile diagram, it is endothermic.
Hope this helps! :)
It would be an endothermic reaction because recall enthalpy is a state function, where the overall change in independent of the path.
Thus, if the products are above the reactants in terms of enthalpy on an energy profile diagram, it is endothermic.
Hope this helps! :)
- Mon Jan 25, 2021 10:17 am
- Forum: Phase Changes & Related Calculations
- Topic: Sublimation
- Replies: 13
- Views: 1623
Re: Sublimation
Hi, Sublimation is defined as a phase change from solid to gas (e.g. dry ice subliming into carbon dioxide gas). It is considered endothermic because energy is being invested into the system in order to disrupt the intermolecular forces between the particles in a solid in order to become a gas. Hope...
- Mon Jan 25, 2021 10:15 am
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: endo/exothermic reactions
- Replies: 13
- Views: 420
Re: endo/exothermic reactions
Hi, If a reaction requires heat, then it is considered an endothermic reaction. While breaking bonds is considered endothermic, a chemical reaction involves BOTH breaking and forming bonds. Where we differentiate between endothermic and exothermic is the net change in heat, or in other words, compar...
- Mon Jan 18, 2021 12:11 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Inert Gas and Pressure
- Replies: 5
- Views: 246
Re: Inert Gas and Pressure
Hi,
Yes! The addition of another gas (typically an inert gas) will lead to more overall collisions with the walls of the container, making the overall pressure increase.
Hope this helps! :)
Yes! The addition of another gas (typically an inert gas) will lead to more overall collisions with the walls of the container, making the overall pressure increase.
Hope this helps! :)
- Mon Jan 18, 2021 12:10 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: When would K be unchanged?
- Replies: 31
- Views: 1058
Re: When would K be unchanged?
Hi,
The only change which would change the value of K would be temperature (we'll learn why when we study kinetics).
Changes in concentrations, partial pressures, addition of catalysts, changes in volume, or addition of noble gases have no effect.
Hope this helps! :)
The only change which would change the value of K would be temperature (we'll learn why when we study kinetics).
Changes in concentrations, partial pressures, addition of catalysts, changes in volume, or addition of noble gases have no effect.
Hope this helps! :)
- Mon Jan 18, 2021 12:08 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Total Pressure
- Replies: 26
- Views: 1831
Re: Total Pressure
Hi, Total pressure is the sum of all the partial pressures of the all the gases in a system. For example, let's say you have a reaction vessel where the partial pressure of He is 5.0 atm and the partial pressure of Xe is 10.0 atm. Thus, the total pressure of the system would be 15.0 atm. Hope this h...
- Mon Jan 18, 2021 12:07 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: equilibrium shifts: left of right?
- Replies: 13
- Views: 647
Re: equilibrium shifts: left of right?
Hi,
Assuming the initial concentrations of reactants and products are equilibrium concentrations, then the reaction should proceed to the right.
Hope this helps! :)
Assuming the initial concentrations of reactants and products are equilibrium concentrations, then the reaction should proceed to the right.
Hope this helps! :)
- Mon Jan 18, 2021 12:06 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: endothermic vs exothermic
- Replies: 16
- Views: 682
Re: endothermic vs exothermic
Hi,
A reaction is endothermic if the delta H is positive.
A reaction is exothermic if the delta H is negative.
Hope this helps! :)
A reaction is endothermic if the delta H is positive.
A reaction is exothermic if the delta H is negative.
Hope this helps! :)
- Mon Jan 11, 2021 1:26 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Change in Temp
- Replies: 9
- Views: 392
Re: Change in Temp
Hi,
Yes. If the enthalpy (delta H) is negative, the reaction is exothermic. If the enthalpy (delta H) is positive, the reaction is endothermic.
Hope this helps! :)
Yes. If the enthalpy (delta H) is negative, the reaction is exothermic. If the enthalpy (delta H) is positive, the reaction is endothermic.
Hope this helps! :)
- Mon Jan 11, 2021 1:24 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: change in K
- Replies: 22
- Views: 812
Re: change in K
Hi,
Yes, temperature is the only change which affects the value of the equilibrium constant K.
Hope this helps! :)
Yes, temperature is the only change which affects the value of the equilibrium constant K.
Hope this helps! :)
- Mon Jan 11, 2021 1:23 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Coefficients for eq constant
- Replies: 9
- Views: 560
Re: Coefficients for eq constant
Hi,
You would raise those coefficients to their respective product, assuming they are in the gaseous or aqueous phase for the equilibrium constant.
Hope this helps! :)
You would raise those coefficients to their respective product, assuming they are in the gaseous or aqueous phase for the equilibrium constant.
Hope this helps! :)
- Mon Jan 11, 2021 1:22 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Adding Helium
- Replies: 10
- Views: 866
Re: Adding Helium
Hi,
Adding helium will increase the overall pressure of the system, but it will not increase the individual partial pressures of the other gases enclosed in the system.
This is why there is not shift when it is added.
Hope this helps! :)
Adding helium will increase the overall pressure of the system, but it will not increase the individual partial pressures of the other gases enclosed in the system.
This is why there is not shift when it is added.
Hope this helps! :)
- Mon Jan 11, 2021 1:20 pm
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: H2O
- Replies: 44
- Views: 1891
Re: H2O
Hi,
We would only include H2O in the gaseous phase, as in the equilibrium constant.
We would not include H2O in the solid or liquid phase as they are pure substances.
Hope this helps! :)
We would only include H2O in the gaseous phase, as in the equilibrium constant.
We would not include H2O in the solid or liquid phase as they are pure substances.
Hope this helps! :)
- Mon Jan 04, 2021 12:21 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Equilibrium Constants
- Replies: 15
- Views: 862
Re: Equilibrium Constants
Hi,
Yes, the balanced chemical equation is required to find K.
Note, however, the stoichiometric coefficients must be to the lowest factor and must be whole numbers. For instance, don't put 0.5 as a coefficient or if the coefficients are 2 and 4, simplify to 1 and 2.
Hope this helps! :)
Yes, the balanced chemical equation is required to find K.
Note, however, the stoichiometric coefficients must be to the lowest factor and must be whole numbers. For instance, don't put 0.5 as a coefficient or if the coefficients are 2 and 4, simplify to 1 and 2.
Hope this helps! :)
- Mon Jan 04, 2021 12:19 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: If K is large...
- Replies: 11
- Views: 1031
Re: If K is large...
Hi, Note, the equilibrium constant is just an arbitrary number. The larger K is, the more it favors the products. (K > 1) The smaller K is, the more it favors the reactants. (K < 1) However, when a reaction is at equilibrium, because the constant is just an arbitrary number the concentrations of rea...
- Mon Jan 04, 2021 12:14 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Reaction Direction
- Replies: 19
- Views: 957
Re: Reaction Direction
Hi, In order to determine the predominant direction of a reaction, it depends on how you phrase it. Whether you are talking about the relative magnitudes of the K value (1) or a response in doing something to perturb the system (2). Note, whether the reaction is a decomposition or synthesis reaction...
- Mon Jan 04, 2021 12:05 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: KC vs KP [ENDORSED]
- Replies: 6
- Views: 329
Re: KC vs KP [ENDORSED]
Hi, It entirely depends on the context on what you are given. If you are given any information which may lead you to find concentrations ( mol, M, mmol, L, mL, g, mg ), use K_c . If you are given any information which may lead you to find partial pressures ( PV = nRT, atm, bars, mm Hg ), then use K_...
- Mon Jan 04, 2021 11:40 am
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: Sapling #7
- Replies: 6
- Views: 219
Re: Sapling #7
Hi, Note, it is important to remember the equilibrium constant K is dependent only on temperature. Changes to initial conditions such as initial concentrations, initial partial pressures, or introductions of catalysts do not affect the value of K . When the temperature is increased for the system, i...
- Mon Dec 07, 2020 1:22 pm
- Forum: Identifying Acidic & Basic Salts
- Topic: Conjugate Bases
- Replies: 3
- Views: 195
Re: Conjugate Bases
Hi, A conjugate base is what the original acid turns into when it gives up a proton or H+. For instance, consider the following reaction: HA(aq)+H_2O(l) \leftrightharpoons A^-(aq) + H_3O^+(aq) In the context of the equation, HA(aq) represents a weak acid. When HA give...
- Mon Dec 07, 2020 1:17 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Dentates
- Replies: 7
- Views: 311
Re: Dentates
Hi,
In order to determine the denticity of a ligand you would need to look at the not only just the available lone pairs needed to create a coordinate covalent bond, but also the spacing.
For example, this is why H2O is monodentate even though it has two lone pairs.
Hope this helps! :)
In order to determine the denticity of a ligand you would need to look at the not only just the available lone pairs needed to create a coordinate covalent bond, but also the spacing.
For example, this is why H2O is monodentate even though it has two lone pairs.
Hope this helps! :)
- Mon Dec 07, 2020 1:14 pm
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: Cl- not effecting pH
- Replies: 5
- Views: 450
Re: Cl- not effecting pH
Hi, Na+ does not affect pH as the electrostatic interactions between Na+ and H2O are not significant enough to yield a coordination compound, which would have made the pH more acidic. Cl- does not affect pH because it is the conjugate base of a strong acid. Even if Cl- were to react with H2O to yiel...
- Mon Dec 07, 2020 8:06 am
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Coordination Numbers
- Replies: 11
- Views: 543
Re: Coordination Numbers
Hi,
The central atom in a coordination compound is always the transition metal.
Hope this helps! :)
The central atom in a coordination compound is always the transition metal.
Hope this helps! :)
- Mon Dec 07, 2020 8:04 am
- Forum: Properties & Structures of Inorganic & Organic Acids
- Topic: Oxoacids?
- Replies: 4
- Views: 271
Re: Oxoacids?
Hi, Oxoacids are acids containing an oxygen. (i.e. HNO3 for example). They are most commonly found in organic acids, such as a acetic acid. (i.e. HC2H3O2) In the scope of this course, one of the main things you'll need to know is the effect of the additional number of oxygen atoms on an acid in term...
- Mon Nov 30, 2020 8:39 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Polarity and Dipole Moments
- Replies: 4
- Views: 196
Re: Polarity and Dipole Moments
Hi,
Whenever we term a dipole as "cancelling out," we mean that the polar bonds are oriented in such a way that the molecule is symmetric (I.e. tetrahedral). This effectively removes the dipole from the molecule, making it nonpolar.
Hope this helps! :)
Whenever we term a dipole as "cancelling out," we mean that the polar bonds are oriented in such a way that the molecule is symmetric (I.e. tetrahedral). This effectively removes the dipole from the molecule, making it nonpolar.
Hope this helps! :)
- Mon Nov 30, 2020 8:36 am
- Forum: Bond Lengths & Energies
- Topic: LDF Bond Strength
- Replies: 11
- Views: 916
Re: LDF Bond Strength
Hi,
The reason the list of LDFs are listed as it is, is because the size of I2 is far larger than that of the other diatomic molecules with the most number of electrons. This results in a greater polarizability and in turn, leads to stronger LDFs.
Hope this helps! :)
The reason the list of LDFs are listed as it is, is because the size of I2 is far larger than that of the other diatomic molecules with the most number of electrons. This results in a greater polarizability and in turn, leads to stronger LDFs.
Hope this helps! :)
- Mon Nov 30, 2020 8:32 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: polar v nonpolar molecules
- Replies: 30
- Views: 2309
Re: polar v nonpolar molecules
Hi,
Polar molecules tend to have polar bonds which are in an asymmetric molecule, while nonpolar molecules either have only nonpolar bonds or have polar bonds which cancel out.
Hope this helps! :)
Polar molecules tend to have polar bonds which are in an asymmetric molecule, while nonpolar molecules either have only nonpolar bonds or have polar bonds which cancel out.
Hope this helps! :)
- Mon Nov 30, 2020 8:29 am
- Forum: Ionic & Covalent Bonds
- Topic: Polar and Nonpolar
- Replies: 37
- Views: 1677
Re: Polar and Nonpolar
Hi,
You should also take into account the shape of the molecule as the asymmetry/symmetry may cancel out polar bonds.
Hope this helps! :)
You should also take into account the shape of the molecule as the asymmetry/symmetry may cancel out polar bonds.
Hope this helps! :)
- Mon Nov 30, 2020 8:26 am
- Forum: Bond Lengths & Energies
- Topic: London Dispersion Forces
- Replies: 5
- Views: 285
Re: London Dispersion Forces
Hi,
Yes! More bounded atoms imply more electrons, increasing the polarizability of the particle or the strength of the LDFs.
Hope this helps! :)
Yes! More bounded atoms imply more electrons, increasing the polarizability of the particle or the strength of the LDFs.
Hope this helps! :)
- Mon Nov 23, 2020 9:22 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Axial vs Equatorial atoms
- Replies: 8
- Views: 341
Re: Axial vs Equatorial atoms
Hi,
I like the think of the axial atoms as those "pointing upward" in the vertical direction, while equatorial atoms are those "pointing to the side" as with the equator of the Earth.
Hope this helps! :)
I like the think of the axial atoms as those "pointing upward" in the vertical direction, while equatorial atoms are those "pointing to the side" as with the equator of the Earth.
Hope this helps! :)
- Mon Nov 23, 2020 9:19 am
- Forum: Bond Lengths & Energies
- Topic: Higher Melting Point
- Replies: 28
- Views: 2493
Re: Higher Melting Point
Hi, This is because the atomic radius of the iodine atom is far larger than that of the fluorine atom. This leads to increased polarizability, increased LDFs, and increased strength of intermolecular attractions. The more energy required to disrupt these interactions, the higher the temperature need...
- Mon Nov 23, 2020 9:17 am
- Forum: Bond Lengths & Energies
- Topic: Bond Strength in DNA
- Replies: 12
- Views: 753
Re: Bond Strength in DNA
Hi,
Yes! That is correct! The additional hydrogen bond makes the GC attractions stronger!
Hope this helps! :)
Yes! That is correct! The additional hydrogen bond makes the GC attractions stronger!
Hope this helps! :)
- Mon Nov 23, 2020 9:15 am
- Forum: Interionic and Intermolecular Forces (Ion-Ion, Ion-Dipole, Dipole-Dipole, Dipole-Induced Dipole, Dispersion/Induced Dipole-Induced Dipole/London Forces, Hydrogen Bonding)
- Topic: London Forces [ENDORSED]
- Replies: 19
- Views: 774
Re: London Forces [ENDORSED]
Hi,
Yes! LDFs are based on the polarizability of a given particle, which are determined by electrons. Due to how every molecule has electrons, LDFs are exhibited everywhere!
Hope this helps! :)
Yes! LDFs are based on the polarizability of a given particle, which are determined by electrons. Due to how every molecule has electrons, LDFs are exhibited everywhere!
Hope this helps! :)
- Mon Nov 23, 2020 9:12 am
- Forum: Bond Lengths & Energies
- Topic: Melting Point
- Replies: 12
- Views: 562
Re: Melting Point
Hi, Before we can deduce which element has a higher melting point, we need to understand what determines the melting point. As the melting point is the temperature at which a substance transitions from a solid into a liquid, you can think of the temperature as an amount of energy (i.e. higher temper...
- Mon Nov 16, 2020 7:41 am
- Forum: Dipole Moments
- Topic: London Dispersion Forces
- Replies: 10
- Views: 830
Re: London Dispersion Forces
Hi, It is important to note that London Dispersion Forces arise from electrons. As the delocalized electrons of a given particle are moving around at any given moment in time, if you were to take a snapshot over a given interval you would see that at some point the electrons would be dispersed in su...
- Mon Nov 16, 2020 7:38 am
- Forum: Ionic & Covalent Bonds
- Topic: Bond Length
- Replies: 6
- Views: 751
Re: Bond Length
Hi,
The relationship is that bond length is inversely proportional to bond strength. Therefore, if you are comparing two bonds and one is shorter than the prior, the latter has a higher bond energy.
Hope this helps! :)
The relationship is that bond length is inversely proportional to bond strength. Therefore, if you are comparing two bonds and one is shorter than the prior, the latter has a higher bond energy.
Hope this helps! :)
- Mon Nov 16, 2020 7:37 am
- Forum: Lewis Structures
- Topic: Hydrogen Bonding
- Replies: 12
- Views: 508
Re: Hydrogen Bonding
Hi, This is because since the electronegativities of nitrogen (N), oxygen (O), and fluorine (F) are so large in magnitude, they are often singled out from the typical dipole-dipole classification when covalently bonded to hydrogen as a hydrogen bond. However, because carbon's (C) electronegativity i...
- Mon Nov 16, 2020 7:33 am
- Forum: Dipole Moments
- Topic: Which interactions are intermolecular?
- Replies: 7
- Views: 342
Re: Which interactions are intermolecular?
Hi,
Yes! Those are all considered intermolecular forces as they are "between" two species!
Hope this helps! :)
Yes! Those are all considered intermolecular forces as they are "between" two species!
Hope this helps! :)
- Mon Nov 16, 2020 7:32 am
- Forum: Lewis Structures
- Topic: Lewis acids and bases
- Replies: 23
- Views: 771
Re: Lewis acids and bases
Hi,
A Lewis acid accepts an electron pair, while a Lewis base donates an electron pair.
Hope this helps! :)
A Lewis acid accepts an electron pair, while a Lewis base donates an electron pair.
Hope this helps! :)
- Mon Nov 09, 2020 12:30 pm
- Forum: Ionic & Covalent Bonds
- Topic: negative energies for attractive interactions
- Replies: 7
- Views: 264
Re: negative energies for attractive interactions
Hi, Well, before we can understand why attractive interactions yield negative energies we need to first answer one question: Why do atoms form these interactions? In nature, you can think of most particles as being "unstable." Generally, when atoms or molecules are in an unstable state the...
- Mon Nov 09, 2020 12:20 pm
- Forum: Electronegativity
- Topic: Delta negative and delta positive?
- Replies: 8
- Views: 4517
Re: Delta negative and delta positive?
Hi, So, recall the delta negative the delta positive symbols are used to denote a separation of charge in an atom. This separation of charge is based on the electronegativities or "pulling power" of an atom's nuclei for electrons. So, if an atom has a high electronegativity, it really want...
- Mon Nov 09, 2020 12:16 pm
- Forum: Dipole Moments
- Topic: London dispersion
- Replies: 4
- Views: 154
Re: London dispersion
Hi,
Yes! Recall, London Dispersion Forces (LDFs) originate due to the temporary displacement of electrons, resulting in a separation of charge in the overall molecule as a result of delocalized electrons. Therefore, LDFs are present in all particles due to the presence of electrons.
Hope this helps!
Yes! Recall, London Dispersion Forces (LDFs) originate due to the temporary displacement of electrons, resulting in a separation of charge in the overall molecule as a result of delocalized electrons. Therefore, LDFs are present in all particles due to the presence of electrons.
Hope this helps!
- Mon Nov 09, 2020 12:14 pm
- Forum: Bond Lengths & Energies
- Topic: bond lengths
- Replies: 9
- Views: 423
Re: bond lengths
Hi,
Bond length is inversely proportional to bond strength. So, let's say you were given two bonds of two arbitrary molecules for "X-X" and "X=X." Because the double bond in the second molecule is stronger, the bond length must be shorter.
Hope this helps! :)
Bond length is inversely proportional to bond strength. So, let's say you were given two bonds of two arbitrary molecules for "X-X" and "X=X." Because the double bond in the second molecule is stronger, the bond length must be shorter.
Hope this helps! :)
- Mon Nov 09, 2020 12:12 pm
- Forum: Ionic & Covalent Bonds
- Topic: Hydrogen Bonds [ENDORSED]
- Replies: 9
- Views: 502
Re: Hydrogen Bonds [ENDORSED]
Hi, Yes! Hydrogen bonding does originate from a separation of charge (i.e. partial positives and partial negatives) within the molecules in question, as does the case of dipole-dipole interactions. Hydrogen bonding, however, is simply a more perturbed separation of charge (or a stronger variant) due...
- Mon Nov 02, 2020 12:33 pm
- Forum: Formal Charge and Oxidation Numbers
- Topic: Electron Configuration
- Replies: 10
- Views: 544
Re: Electron Configuration
Hi, Typically, when we are doing electron configurations, we number the electrons in order of lowest energy to highest energy. You can think of it as having the principal quantum number be listed in order of consequence (n=1, 2, 3... => 1s 2s 3s 4s) and in order of the subshells (s then p then d the...
- Mon Nov 02, 2020 12:31 pm
- Forum: Ionic & Covalent Bonds
- Topic: Non Metals
- Replies: 10
- Views: 701
Re: Non Metals
Hi, There are multiple ways to think about this concept, but I'm going to answer it in terms of electron configurations. This is due to how nonmetals (i.e. the elements near the right-most end of the periodic table), as with other elements, have a tendency to reach a noble gas configuration in order...
- Mon Nov 02, 2020 12:25 pm
- Forum: SI Units, Unit Conversions
- Topic: Converting equations
- Replies: 16
- Views: 767
Re: Converting equations
Hi, A common tip I would use is to first write down what equations you will be working with right in front of you. From there, I would be sure to write out each step in the process without skipping any details as I am plugging in equations. Finally, I would check at the end to see if the units of bo...
- Mon Nov 02, 2020 12:22 pm
- Forum: Ionic & Covalent Bonds
- Topic: Ionic vs Covalent
- Replies: 32
- Views: 43263
Re: Ionic vs Covalent
Hi,
Generally, we consider ionic bonds to be stronger than covalent bonds.
Hope this helps! :)
Generally, we consider ionic bonds to be stronger than covalent bonds.
Hope this helps! :)
- Mon Nov 02, 2020 12:18 pm
- Forum: Formal Charge and Oxidation Numbers
- Topic: Why do we use formal charge?
- Replies: 14
- Views: 1902
Re: Why do we use formal charge?
Hi, Whenever we are constructing Lewis Structures, often times we arrive at situations where there is more than one valid structure. Note, I am not referring to resonance, I am referring to a scenario of whether or not you should have all singles bonds or include a double bond here and there as with...
- Mon Oct 26, 2020 3:37 pm
- Forum: Quantum Numbers and The H-Atom
- Topic: Px Py Pz
- Replies: 4
- Views: 226
Re: Px Py Pz
Hi, In the context of electron configuration and orbitals, let's break down what "px, py, and pz" means. The "p" in front of each portion of the question indicates the subshell/state the electron is occupying. Thus, the electron is begin associated with the p-subshell/state. The ...
- Mon Oct 26, 2020 3:33 pm
- Forum: Empirical & Molecular Formulas
- Topic: Dealing with Diatomic Elements
- Replies: 14
- Views: 1299
Re: Dealing with Diatomic Elements
Hi, Whenever you are doing empirical formula problems and simplifying the ratios of the moles of its components, always be sure (for the sake of ease) to use moles of just the atom, not it's elemental state. For instance, use moles of N instead of moles of N2 or use moles of O instead of moles of O2...
- Mon Oct 26, 2020 3:28 pm
- Forum: Photoelectric Effect
- Topic: Photoelectric Effect [ENDORSED]
- Replies: 4
- Views: 256
Re: Photoelectric Effect [ENDORSED]
Hi, In the context of the chapter, recall that we are studying electromagnetic radiation. By the name, it implies the radiation were are studying exhibits an electric field ("electro-") and a magnetic field ("-magnetic). Now, you can think of an electric field as an array of an infini...
- Mon Oct 26, 2020 3:24 pm
- Forum: Heisenberg Indeterminacy (Uncertainty) Equation
- Topic: How to Calculate Uncertainty
- Replies: 6
- Views: 270
Re: How to Calculate Uncertainty
Hi, With regards to uncertainty in position, if you are not solving for it, the problem will most likely give you the value. However, they could give it to you in a variety of ways. For instance, in terms of the "atom in a box" model, they could give you a statement such as "The uncer...
- Mon Oct 26, 2020 3:18 pm
- Forum: Properties of Light
- Topic: Lyman VS Balmer series
- Replies: 5
- Views: 228
Re: Lyman VS Balmer series
Hi, Yes that is correct! Recall in the context of hydrogen (H) atoms, electrons may leave the ground state (n=1) by getting excited by an incoming photon from a source of electromagnetic radiation. Now, in our discussion of Lyman and Balmer series we are interested in which energy level the excited ...
- Mon Oct 19, 2020 1:07 pm
- Forum: Bohr Frequency Condition, H-Atom , Atomic Spectroscopy
- Topic: Rydberg Equation and Empirical Equation
- Replies: 4
- Views: 212
Re: Rydberg Equation and Empirical Equation
Hi,
Yes! That is correct! The Rydberg equation is only appropriate for working with electron transitions in the hydrogen (H) atom. In systems differing from hydrogen (H), as with carbon (C) or nitrogen (N), an alternate equation must be used.
Hope this helps! :)
Yes! That is correct! The Rydberg equation is only appropriate for working with electron transitions in the hydrogen (H) atom. In systems differing from hydrogen (H), as with carbon (C) or nitrogen (N), an alternate equation must be used.
Hope this helps! :)
- Mon Oct 19, 2020 1:05 pm
- Forum: Photoelectric Effect
- Topic: Units of the Work Function
- Replies: 7
- Views: 148
Re: Units of the Work Function
Hi,
It depends on the problem, but in most cases we will be working with energy in terms of one particle (i.e. photons or electrons as in the photoelectric experiment).
Hope this helps! :)
It depends on the problem, but in most cases we will be working with energy in terms of one particle (i.e. photons or electrons as in the photoelectric experiment).
Hope this helps! :)
- Mon Oct 19, 2020 1:03 pm
- Forum: Photoelectric Effect
- Topic: Light Intensity
- Replies: 23
- Views: 455
Re: Light Intensity
Hi, Yes! As the intensity of the light increases, we associate that property as increasing in brightness! However, don't forget increasing intensity increases the number of photons! For example, let's say we have two intensities I_1 and I_2 , where I_1 > I_2 . Thus, I_1 would have more photons than ...
- Mon Oct 19, 2020 9:58 am
- Forum: Properties of Electrons
- Topic: Lyman vs. Balmer series
- Replies: 20
- Views: 1857
Re: Lyman vs. Balmer series
Hi, The main difference between the Lyman Series and the Balmer Series during electron excitation in the hydrogen (H) atom is based on the wavelength of light (and subsequent energy) when the excited electron returns to the ground state. For the Lyman Series, electrons return to the principal energy...
- Mon Oct 19, 2020 9:54 am
- Forum: Properties of Electrons
- Topic: Energy per Photon
- Replies: 7
- Views: 194
Re: Energy per Photon
Hi,
Personally, I would approach with caution in the context of the problem. Depending on if the ejected electron has 0 kinetic energy (KE) or an excess amount, the energy of the incoming light may be exactly the same as the work function or be greater.
Hope this helps!
Personally, I would approach with caution in the context of the problem. Depending on if the ejected electron has 0 kinetic energy (KE) or an excess amount, the energy of the incoming light may be exactly the same as the work function or be greater.
Hope this helps!
- Mon Oct 12, 2020 7:58 pm
- Forum: Balancing Chemical Reactions
- Topic: Balancing equations.
- Replies: 35
- Views: 2492
Re: Balancing equations.
Hi, When I was in high school, a good tip I used when balancing equations was to first rewrite the equation on a separate piece of paper and ensure I wrote it down correctly. Next, I would start balancing whatever was the most convenient first (i.e. the atom in least amount) and then proceed from th...
- Mon Oct 12, 2020 7:54 pm
- Forum: Balancing Chemical Reactions
- Topic: Law of Conservation with Exothermic/Endothermic Reactions
- Replies: 11
- Views: 722
Re: Law of Conservation with Exothermic/Endothermic Reactions
Hi, With regards to the law of conservation of mass, we only factor in portions of the problem which are considered mass (kg, mg, ng, &c.). Heat, however, is not considered as mass, but as energy as when butane is combusted. Thus, the law of conservation of mass in a closed system still takes in...
- Mon Oct 12, 2020 7:50 pm
- Forum: Empirical & Molecular Formulas
- Topic: Finding Empirical Formula
- Replies: 10
- Views: 441
Re: Finding Empirical Formula
Hi, The reason he had to multiply the ratio to get the empirical formula is because when we write out a chemical formula in general, it is not preferred to have fractional numbers (i.e. N_1.5 is not appropriate, while N_2 is). Thus, we need to ensure that 1.33 is multiplied accordingly to get a numb...
- Mon Oct 12, 2020 7:47 pm
- Forum: Properties of Electrons
- Topic: protons and electrons
- Replies: 33
- Views: 2486
Re: protons and electrons
Hi, The mass of a proton and a neutron are approximately the same, which is about 1 amu (atomic mass unit). The mass of an electron is far less than that of a proton or neutron, which is about 0.0005 amu (atomic mass unit). This is why when we do stoichiometry problems, we approximate the molar mass...
- Mon Oct 12, 2020 7:43 pm
- Forum: Balancing Chemical Reactions
- Topic: Molar Mass
- Replies: 23
- Views: 1825
Re: Molar Mass
Hi, Honestly, it depends on the situation. If you were provided a problem which gives you a specific variation of the molar mass of an atom, I would use that. If during the exam you were given an entire periodic table for the length of the test, I would use that. However, despite the variation, as l...
- Mon Oct 05, 2020 3:36 pm
- Forum: Balancing Chemical Reactions
- Topic: Stoichemetric Coeffiecients
- Replies: 12
- Views: 451
Re: Stoichemetric Coeffiecients
Hi, When dealing with a chemical equation, the stoichiometric coefficient refers to the number in front of the elements/compounds/ions/&c in the balanced chemical equation. With regards to balancing, sometimes it may be useful to use fractional numbers (i.e. 13/2) in the process of balancing, bu...
- Mon Oct 05, 2020 3:32 pm
- Forum: SI Units, Unit Conversions
- Topic: SI Units in Answer?
- Replies: 15
- Views: 330
Re: SI Units in Answer?
Hi, With regards to your question on SI Units, it entirely depends on the problem. For instance, if the problem was a dilution equation and it gave you all of the quantities in terms of molarity (M or mol/L) and liters (L), but asked for an answer in milliliters (mL), use mL in your final answer. Or...
- Mon Oct 05, 2020 3:25 pm
- Forum: Balancing Chemical Reactions
- Topic: Balancing chemical equations involving combustion
- Replies: 15
- Views: 482
Re: Balancing chemical equations involving combustion
Hi,
Yes, I believe that is true. In the example the professor provided, it is termed as a "combustion reaction." This implies the substance which undergoes combustion (in this case butane) reacts with oxygen (O2) to form carbon dioxide (CO2) and water vapor (H2O).
Yes, I believe that is true. In the example the professor provided, it is termed as a "combustion reaction." This implies the substance which undergoes combustion (in this case butane) reacts with oxygen (O2) to form carbon dioxide (CO2) and water vapor (H2O).
- Mon Oct 05, 2020 3:21 pm
- Forum: Molarity, Solutions, Dilutions
- Topic: Units for Dilution Equation [ENDORSED]
- Replies: 23
- Views: 2212
Re: Units for Dilution Equation [ENDORSED]
Hi, When using the dilution equation "M1V1 = M2V2" it is ensured to be used with the units of moles (mol) per liters of solution (L) as in "mol/L" for Molarity and liters (L) for Volume. With regards to mL, if the question asks for milliliters (mL) for an answer, be sure to use l...