Search found 37 matches
- Thu Mar 16, 2023 1:54 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Ionization energy and enthalpy of ionization
- Replies: 3
- Views: 509
Re: Ionization energy and enthalpy of ionization
Hi! Just to add on to the previous answer, Ionization energy (amount of energy needed to remove an electron) is a periodic trend. You can predict the ionization energy of one element to the next using the trends. Ionization energy increases from left to right across a period and decreases down a col...
- Thu Mar 16, 2023 1:40 pm
- Forum: Balancing Redox Reactions
- Topic: oxidation number
- Replies: 18
- Views: 1525
Re: oxidation number
HI!
Just like O2, the oxidation number of O3 is 0
Just like O2, the oxidation number of O3 is 0
- Tue Mar 14, 2023 8:19 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Week 5- Isolated system: Adiabatic
- Replies: 5
- Views: 177
Re: Week 5- Isolated system: Adiabatic
An isolated system is not only no energy flow in or out of the system, but it also means that there is no transfer of matter in or out of the system. Thus an adiabatic system would follow the no energy transfer requirement of a system, but that doesn't necessarily mean that there is no transfer of m...
- Tue Mar 14, 2023 8:10 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Week 5- Volume and Entropy
- Replies: 3
- Views: 142
Re: Week 5- Volume and Entropy
Hi! Entropy increases when the volume increases because there is more space for the molecules to move and different ways they can collide. Basically, their arrangement becomes more random. Spontaneous reactions mean that they can occur without an input of energy, they just happen. The second law of ...
- Tue Mar 14, 2023 8:03 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Week 4- The Universe is an Isolated System?
- Replies: 4
- Views: 338
Re: Week 4- The Universe is an Isolated System?
An isolated system is one in which no energy and matter can be transferred. Thus, those who consider the universe to be an isolated system say it is because there is no matter or energy exchange with it's surroundings. It was mentioned in lecture that a truly isolated system would technically be imp...
- Tue Mar 14, 2023 7:58 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Week 3- Enthalpy methods and phase changes
- Replies: 2
- Views: 113
Re: Week 3- Enthalpy methods and phase changes
Hi!
I find that the best formula I like to use for phase changes are the ones with q. The ones that are q(phase change)=mass*enthalpy of fusion/vaporization.
I find that the best formula I like to use for phase changes are the ones with q. The ones that are q(phase change)=mass*enthalpy of fusion/vaporization.
- Tue Mar 14, 2023 7:55 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Week 4- Isolated Systems
- Replies: 3
- Views: 124
Re: Week 4- Isolated Systems
Well, the shortest answer to your second question is that it is actually technically impossible to have a perfectly isolated system in which both matter and energy cannot transfer through, so this actually does not occur naturally. However, some other examples of isolated systems (which again is deb...
- Tue Mar 14, 2023 7:53 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: Versions of Arrhenius Equation
- Replies: 3
- Views: 88
Re: Versions of Arrhenius Equation
Hi!
They should be the same because to isolate k from lnk, you would multiply by e and that would give you the leftmost equation you listed. So the shortest answer is yes, you can use both and get the same answer. :)
They should be the same because to isolate k from lnk, you would multiply by e and that would give you the leftmost equation you listed. So the shortest answer is yes, you can use both and get the same answer. :)
- Tue Mar 14, 2023 7:42 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: Arrhenius Equation Frequency Factor
- Replies: 1
- Views: 112
Re: Arrhenius Equation Frequency Factor
The Arrehenius Equation formula is as follows:
k=A(e^-Ea/RT)
In this formula, A is the frequency factor. A represents the the number of collisions with the correct rotation that allows the reaction to commence. Hope that helped!
k=A(e^-Ea/RT)
In this formula, A is the frequency factor. A represents the the number of collisions with the correct rotation that allows the reaction to commence. Hope that helped!
- Tue Mar 14, 2023 7:38 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: Steady State Approximation and Pre-Equilibrium
- Replies: 2
- Views: 104
Re: Steady State Approximation and Pre-Equilibrium
Hi! Here's my understanding of the two: Steady state: consider the the concentration of an equilibrium to be a constant value in a rate limiting step of a reaction (slow step). So, when you take the derivative, d[intermediate concentration]/dt which gives you the rate of change of concentration over...
- Tue Mar 14, 2023 7:17 pm
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: UA session worksheet question
- Replies: 2
- Views: 108
Re: UA session worksheet question
Hi! My first instinct is to tell you that since Ka is just the acid dissociation constant, it is the same as the K of the dissociation equation. So I'm not sure if there's more to the problem that is not in this picture (an overall balanced equation), but what I believe I would try to do (to make su...
- Sun Mar 05, 2023 10:51 pm
- Forum: Balancing Redox Reactions
- Topic: Half Reactions
- Replies: 3
- Views: 166
Re: Half Reactions
Hi! other people went into great detail :), but i find short supplemental summaries helpful too, so i offer the following: So you use H2O to balance oxygen atoms (add the H2O to the side opposite of the oxygen atoms). Electrons are used to balance charges (and are usually added to the side with the ...
- Sun Mar 05, 2023 9:03 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: E cell, K and Delta G
- Replies: 5
- Views: 1601
Re: E cell, K and Delta G
Hi! The equations I find helpful in thinking through these relationships are deltaG° = -RTIn (K) deltaG° = -nFE°cell E°cell = (deltaG°)/nF when K=1 (system is at equilibrium), delta G° and E°cell are equal to zero. For delta G, it is zero because K=1 and ln(K) = ln1=0. Since the lnK term is multipli...
- Sun Mar 05, 2023 8:35 pm
- Forum: Balancing Redox Reactions
- Topic: Adding in H2O when balancing redox reactions
- Replies: 3
- Views: 128
Re: Adding in H2O when balancing redox reactions
Hello! The shortest answer to your question is that you introduce water in a half reaction in order to balance the oxygen atoms. Like the others said, first you balance the non hydrogen and oxygen atoms. Then you balance the oxygen atoms by adding water to the opposite side. The method I choose to u...
- Sun Feb 19, 2023 11:40 pm
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: Value of R
- Replies: 17
- Views: 743
Re: Value of R
(Like so many people said lol) R depends on the units of pressure (and volume) in the problem. Because values of R are usually written with the units (V*P)/(mol*Temp-in Kelvin) the most common different values are thus (assuming V is in Liters): atmospheric pressure at sea level (atm) 0.082057338 L....
- Sun Feb 19, 2023 11:34 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Entropy
- Replies: 2
- Views: 71
Re: Entropy
Some other examples of extensive properties (dependent on the amount of substance present): volume, heat capacity (heat required is extensive), and mass Some other examples of intensive properties (not dependent on the amount of substance present): specific & molar heat capacities, density, temp...
- Sun Feb 19, 2023 10:41 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Why does heat cause a worse burn than boiling water at the same temp?
- Replies: 8
- Views: 402
Re: Why does heat cause a worse burn than boiling water at the same temp?
It is because steam releases more energy onto skin than hot liquid water. This is because steam had energy (heat) added to it, not only to raise it's temperature, but also to vaporize it. Hot liquid water of the same temperature has less energy because there was no energy put into a phase change. Th...
- Sun Feb 19, 2023 10:34 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: irreversible process
- Replies: 4
- Views: 106
Re: irreversible process
Hi!
The change in surroundings always 0 because the final and initial entropies of the surroundings are equal. Thus their difference is zero. This is because energy cannot be added or taken from the surroundings; the entropy is inside the system and does not transfer to surroundings.
The change in surroundings always 0 because the final and initial entropies of the surroundings are equal. Thus their difference is zero. This is because energy cannot be added or taken from the surroundings; the entropy is inside the system and does not transfer to surroundings.
- Sun Feb 12, 2023 8:55 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Isolated System
- Replies: 24
- Views: 481
Re: Isolated System
No, by definition, an isolated system is purposefully insulated so that energy cannot flow in and out. ~~Technically~~ though, it was mentioned in a lecture that its impossible to completely prevent energy from flowing between systems and surroundings, but for this class, we just need to know: isola...
- Sun Feb 12, 2023 8:46 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Hess's Law for Thermodynamics
- Replies: 6
- Views: 191
Re: Hess's Law for Thermodynamics
Hi! When you are doing Hess's law for thermodynamic equations such as ∆H, you add the ∆H values. When having to increase the mole ratio of one reaction to match the overall equation, you multiply that constant to that reaction’s ∆H value. Meaning, if you double the mole ratio of an equation, make su...
- Sun Feb 05, 2023 9:35 pm
- Forum: Phase Changes & Related Calculations
- Topic: Entropy
- Replies: 4
- Views: 137
Re: Entropy
Entropy is the amount of disorder in a system. Changes in entropy are modeled delta S. A negative delta S value is actually indicative of an decrease in the disorder of the system/system becomes more ordered. A positive delta S means that the disorder of a system has increased from a reaction. Somet...
- Sun Feb 05, 2023 9:17 pm
- Forum: Phase Changes & Related Calculations
- Topic: Heating Curve for Water
- Replies: 5
- Views: 270
Re: Heating Curve for Water
Hi, During phase changes, the heat being added is use to break the hydrogen bonds of the water molecules (breaking bonds is endothermic/requires heat). So even though more heat is being added, that heat is not raising the temperature of the water. This is why the heating curve is flat during phase c...
- Fri Feb 03, 2023 3:20 am
- Forum: Phase Changes & Related Calculations
- Topic: Percentage protonated
- Replies: 23
- Views: 797
Re: Percentage protonated
Hi! We are calculating how much the base deprotonated: how the concentration of hydroxide compares to the concentration of the original base. This is calculated by [OH^-]/[Initial Base] *100. Strong bases deprotonate completely and thus have a higher percentage than weaker bases. This concept is hel...
- Fri Feb 03, 2023 3:15 am
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: Effect of pressure
- Replies: 2
- Views: 194
Re: Effect of pressure
Hi! Just wanted to add that it depends on how the change in pressure is created. If it is by pumping in an inert gas like He, there shouldn't be a change in the equilibrium because inert gases are not reactive. If the pressure change was due to a change in volume, like a piston chamber decreasing th...
- Fri Feb 03, 2023 3:10 am
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Reversible process
- Replies: 3
- Views: 391
Re: Reversible process
Hey! I'm not completely sure on this topic, but I did some additional research and here is what I found. a reversible process was defined as being able to be "turned back to such that both the system and the surroundings return to their original states, with no other change anywhere else in the...
- Fri Feb 03, 2023 3:00 am
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Enthalpy
- Replies: 14
- Views: 577
Re: Enthalpy
Hi! Enthalpy is commonly referred to as heat, but is also the energy stored in potential bonds. Change in enthalpy is written as delta H. Exothermic reactions result in a release in heat, so delta H is negative. Heat is released to the surroundings. Forming bonds results in a release of energy and i...
- Thu Feb 02, 2023 8:24 pm
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: Strong Acids and Bases
- Replies: 7
- Views: 444
Re: Strong Acids and Bases
That works! I also like to think about the components of the substance to try to determine if they are a strong acid/strong base. Some strong acids have a hydrogen paired with a halogen (with the exception of F as HF is a weak acid). Ex: HCl, HBr, HI Some strong bases have cations from period one (a...
- Thu Feb 02, 2023 4:13 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Buffers
- Replies: 3
- Views: 193
Re: Buffers
Hi, buffers tend to be weak acids and bases because their disassociation has both forward and reverse reactions. In other words, they do not completely ionize/disassociate, so there are still reactants in the solution once the reaction has reached equilibrium. This means that the reverse reaction ca...
- Sun Jan 22, 2023 6:49 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Kp or Kc
- Replies: 10
- Views: 255
Re: Kp vs Kc
Are Kp and Kc constants? If not, how do we determine the value for them and is a specific variable preferred? Kp and Kc are both equilibrium constants. Kc is an equilibrium constant when the (molar) concentrations of the substances at equilibrium are used in the calculation. Kp is an equilibrium co...
- Sun Jan 22, 2023 6:41 pm
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: K vs KC
- Replies: 27
- Views: 1123
Re: K vs KC
K is generally used to refer to an equilibrium constant Kc is an equilibrium constant when the concentrations of the substances at equilibrium are used in the calculation. Kp is an equilibrium constant when the partial pressures of the substances at equilibrium are used in the calculation. A small d...
- Sun Jan 22, 2023 6:38 pm
- Forum: Ideal Gases
- Topic: Adding equations to find Kc
- Replies: 6
- Views: 330
Re: Adding equations to find Kc
Hi, I'll just add a more visual example to go with the other person's very helpful reply. Example 1 When adding two reactions with different Kc values reaction 1: aA<-->cC Kc=x reaction 2: bB<-->dD Kc=y coupled reaction: aA+bB<-->cC+dD Kc=x*y _________________________________________________________...
- Sun Jan 15, 2023 9:02 pm
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: Re: When Q = K
- Replies: 9
- Views: 210
Re: When Q = K
Hi! Q equals K when a reaction reaches equilibrium. This does not mean there is the same amount of products and reactants! It just means the rate of reaction of the forward and reverse reactions are equal. You can tell when a reaction has reached equilibrium when the concentrations of both the produ...
- Sun Jan 15, 2023 8:57 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Homogeneous and Heterogeneous
- Replies: 3
- Views: 131
Re: Homogeneous and Heterogeneous
Hi! Yes, the phases of the substances in the equation do affect how we calculate K, since we omit substances that are pure liquid and solid form in the equation to calculate K. So, if an equation is homogeneous gas (all reactants and products are gas) then you can include all reactants and products ...
- Fri Jan 13, 2023 11:41 am
- Forum: Student Social/Study Group
- Topic: New Chill Music :)
- Replies: 52
- Views: 3397
Re: New Chill Music :)
I like to just loop Shinunoga E-Wa and it becomes such relaxing background music for my brain while I work.
- Fri Jan 13, 2023 11:37 am
- Forum: Ideal Gases
- Topic: R
- Replies: 19
- Views: 652
Re: R
Assuming you're talking about R in PV=nRT: R depends on the units of pressure (and volume) in the problem. Because values of R are written with the units (V*P)/(mol*Temp-in Kelvin) the most common different values are thus (assuming V is in Liters): Bar 8.3144598 × 10-2 L.bar.K-1.mol-1 Kilopascal (k...
- Fri Jan 13, 2023 11:07 am
- Forum: Student Social/Study Group
- Topic: Fav Candy
- Replies: 40
- Views: 2532
Re: Fav Candy
This huge dark chocolate candy bar from Trader Joes near campus. I really recommend for dark chocolate lovers, but they also have a milk chocolate version. It is literally a pound of chocolate and I love it so much :)
- Fri Jan 13, 2023 11:04 am
- Forum: Student Social/Study Group
- Topic: Post All Chemistry Jokes Here
- Replies: 9651
- Views: 4094758
Re: Post All Chemistry Jokes Here
Q: Why do the other elements call group 18 "the knights of the periodic table"?
A: Because they are the noble gases.
i'm sorry everyone :(
A: Because they are the noble gases.
i'm sorry everyone :(