Search found 87 matches
- Sun Mar 17, 2024 8:32 pm
- Forum: Second Order Reactions
- Topic: Unique Rates
- Replies: 2
- Views: 34
Re: Unique Rates
The unique rate will be the same for ONE unique reaction. Every different reaction will have a different unique rate.
- Sun Mar 17, 2024 8:31 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Delta H and q
- Replies: 5
- Views: 55
Re: Delta H and q
Delta H equals q at constant pressure
- Sun Mar 17, 2024 8:30 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: Arrhenius constant
- Replies: 3
- Views: 23
Re: Arrhenius constant
It's just given. The textbook gives a bunch of components that go into solving for it but we don't need to know that for class
- Sun Mar 17, 2024 8:29 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Textbook 6N.5
- Replies: 2
- Views: 42
Re: Textbook 6N.5
Divide both sides by -0.0257V x 2.303 to get pH= 0.06V/ (2.303)(0.025693V) = 1.0. This is because -log[H+] equals pH, and dividing by this amount will leave us with -log[H+] = 1. Hope this helps!
- Sun Mar 17, 2024 8:27 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Finding EntropY Using Experimental Data
- Replies: 2
- Views: 61
Re: Finding EntropY Using Experimental Data
So entropy approaches zero as the temperature approaches 0 kelvin. I had thought the answer was zero but apparently theres some residual entropy that arises from the fact that the molecule is not a perfect crystal and there is some movement within the molecule. Hope this helps!
- Sun Mar 17, 2024 8:22 pm
- Forum: Second Order Reactions
- Topic: Orders higher than Second
- Replies: 3
- Views: 55
Re: Orders higher than Second
You would do the exact same derivation process that we did in class for the lower orders.
- Sun Mar 17, 2024 8:20 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: Catalyst Addition: Le Chatelier's Principle
- Replies: 3
- Views: 34
Re: Catalyst Addition: Le Chatelier's Principle
the catalyst will increase the rate of both the forward and reverse reaction
- Sun Mar 17, 2024 8:20 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: Catalyst Addition: Le Chatelier's Principle
- Replies: 3
- Views: 34
Re: Catalyst Addition: Le Chatelier's Principle
There is no shift, the reaction will just reach equilibrium faster.
- Sun Mar 17, 2024 8:17 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: qcal=-qreaction
- Replies: 2
- Views: 43
Re: qcal=-qreaction
This is just the same as saying that the q of system = - q of surroundings. the system is the reaction and the surroundings is the calorimeter.
- Sun Mar 17, 2024 8:15 pm
- Forum: Phase Changes & Related Calculations
- Topic: pH
- Replies: 4
- Views: 46
Re: pH
it stands for potential of hydrogen!
- Sun Mar 17, 2024 8:14 pm
- Forum: Phase Changes & Related Calculations
- Topic: catalyst
- Replies: 2
- Views: 32
Re: catalyst
the catalyst is present at the begining and end. the intermediate is produced in the reaction and then consumed
- Sun Mar 17, 2024 8:11 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: Achieve Question 20
- Replies: 3
- Views: 33
Re: Achieve Question 20
You're gonna use the equation k = ae^-ea/rt. write this equation twice (one for cat, one for uncat). Plug in all of the data given. then, divide the two equations (with cat on top). this will give you the answer.
- Sun Mar 17, 2024 8:07 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: Pre-Equilibrum Approach
- Replies: 4
- Views: 29
Re: Pre-Equilibrum Approach
Use the pre equilibrium approach to find the rate law if slow step is not first step because you can’t have an intermediate in the rate law
- Sun Mar 17, 2024 8:05 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: Pre-Equilibrium Approach
- Replies: 1
- Views: 21
Re: Pre-Equilibrium Approach
Write rate law of slow step and set it equal to 1/r times d[R]/dt for rate of product formation Write K = [P]/[R] for step before slow steps and rearrange it so its [intermediate] = K [R] Plug K[R] in for intermediate in d[R]/dt = rk [][] Substitute k/k prime in for K Replace the whole mess of k’s f...
- Sun Mar 17, 2024 8:03 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: Catalyst
- Replies: 3
- Views: 32
Re: Catalyst
the catalyst is present at the begining and end
- Sun Mar 17, 2024 7:57 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: Oxidizing and Reducing Power
- Replies: 3
- Views: 45
Re: Oxidizing and Reducing Power
You look at the reduction potentials in the back of the book. High reduction potential means the species really "wants" electrons, so it has a lot of oxidizing power (and vice versa).
- Sun Mar 17, 2024 7:55 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: delta G and equilibrium
- Replies: 3
- Views: 45
Re: delta G and equilibrium
Delta G = delta g knot minus RTlnK
- Sun Mar 17, 2024 7:53 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Cell potentials
- Replies: 4
- Views: 25
Re: Cell potentials
You should reverse a reduction reaction when an oxidation is occuring. Reduction reactions are presented in the table in the book, so when the half reaction is actually an oxidation you should reverse the reaction to find the oxidation reaction.
- Sun Mar 17, 2024 7:51 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: Slow Step Rate Law
- Replies: 3
- Views: 43
Re: Slow Step Rate Law
Yes, intermediates can be in the rate law of an intermediate step.
- Sat Mar 16, 2024 1:36 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: Hw 14.43 [ENDORSED]
- Replies: 2
- Views: 886
Re: Hw 14.43 [ENDORSED]
Could someone walk me through the rest of the steps to find the answer to this problem? Thank you.
- Sat Mar 16, 2024 10:23 am
- Forum: Kinetics vs. Thermodynamics Controlling a Reaction
- Topic: Equations for kinetics and electrochem
- Replies: 4
- Views: 60
Equations for kinetics and electrochem
What kinetics and electrochem equations (that are not on the equation sheet provided) should we know for the final?
- Sat Mar 16, 2024 10:17 am
- Forum: General Rate Laws
- Topic: K = k/k prime
- Replies: 3
- Views: 40
K = k/k prime
Why does the equilibrium constant K equal k/k prime instead of k prime/ k? I would've thought it would be the latter because K is [products]/[reactants].
- Fri Mar 15, 2024 10:57 am
- Forum: Chem 14B Uploaded Files (Worksheets, etc.)
- Topic: Gabriel Nitro's Workshop - Week 3 (W24)
- Replies: 8
- Views: 890
Re: Gabriel Nitro's Workshop - Week 3 (W24)
Would you mind explaining the answer to #13 part c?
- Fri Mar 15, 2024 10:29 am
- Forum: Interesting Applications: Rechargeable Batteries (Cell Phones, Notebooks, Cars), Fuel Cells (Space Shuttle), Photovoltaic Cells (Solar Panels), Electrolysis, Rust
- Topic: Electrochemical Series
- Replies: 1
- Views: 36
Electrochemical Series
Do we need to memorize the electrochemical series? Or should we just use reduction potential to decide which species will reduce the other one? Is this even going to be on the final?
- Fri Mar 15, 2024 10:27 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Naming for Final
- Replies: 1
- Views: 30
Naming for Final
Do we need to know naming of molecules? Will it be on the final?
- Wed Mar 13, 2024 11:58 am
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: Area under curve
- Replies: 2
- Views: 43
Re: Area under curve
If you integrate a function, it means that you are looking at the area under the curve on the graph. You can see this visually by literally looking at the area under the graphed line. If you have the graphed line, take a pencil and shade everything between that line and the x axis (constrained on th...
- Wed Mar 13, 2024 11:55 am
- Forum: Method of Initial Rates (To Determine n and k)
- Topic: Textbook question 7.1
- Replies: 1
- Views: 24
Re: Textbook question 7.1
A) The molecule ending in Br has the higher activation energy because it takes more energy to be the predominant species (reflected in the fact that it is the predominant species at high temperatures). High temperatures means there is more energy available to overcome the high energy barrier of a hi...
- Sat Mar 09, 2024 12:14 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: Electrochemical series
- Replies: 1
- Views: 27
Electrochemical series
Do we need to memorize the electrochemical series?
- Tue Mar 05, 2024 11:47 am
- Forum: General Rate Laws
- Topic: Graphs
- Replies: 1
- Views: 20
Graphs
What is on the y axis when a graph of a first order reaction is a straight line?
- Tue Mar 05, 2024 11:44 am
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: Calculating Q
- Replies: 2
- Views: 28
Re: Calculating Q
It’s because the anode is generally changing the solid into an aqueous product, producing the product. The cathode is taking the reactant from aqueous solution and changing it into solid.
- Tue Mar 05, 2024 11:40 am
- Forum: General Rate Laws
- Topic: Rate laws
- Replies: 3
- Views: 42
Rate laws
Why are only reactants included in rate laws?
- Tue Mar 05, 2024 11:37 am
- Forum: General Rate Laws
- Topic: K for zero order reaction
- Replies: 1
- Views: 24
K for zero order reaction
What are the units of K when the reaction is zero order?
- Tue Mar 05, 2024 11:34 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Sign of E
- Replies: 2
- Views: 31
Re: Sign of E
E is always positive for galvanic cells because E being positive means the reaction is spontaneous.
- Tue Mar 05, 2024 11:24 am
- Forum: Method of Initial Rates (To Determine n and k)
- Topic: Reaction Order
- Replies: 2
- Views: 29
Re: Reaction Order
A reaction at an order of one will have an increasing rate proportional to the increasing concentration. A reaction at an order of 2 will have an increasing rate that is the squared value of the increasing concentration. (And so forth). A reaction at an order of 0 will not have it’s rate change when...
- Tue Mar 05, 2024 11:22 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Concentration and E
- Replies: 1
- Views: 19
Re: Concentration and E
E knot is under standard conditions, and one of the standard conditions is that everything is at a concentration of one mol
- Tue Mar 05, 2024 11:17 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Electrolytic vs. Galvanic cell
- Replies: 4
- Views: 67
Re: Electrolytic vs. Galvanic cell
Galvanic has positive e cell and is spontaneous, electrolytic is nonspontaneous so it requires energy input.
- Tue Mar 05, 2024 11:08 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Standard Hydrogen Electrode
- Replies: 2
- Views: 23
Standard Hydrogen Electrode
Is the standard hydrogen electrode in the anode or cathode?
- Tue Mar 05, 2024 11:06 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Commas in cell diagrams
- Replies: 1
- Views: 15
Commas in cell diagrams
What do the commas mean in cell diagrams?
- Thu Feb 29, 2024 9:01 pm
- Forum: Balancing Redox Reactions
- Topic: 6k.5 a
- Replies: 1
- Views: 25
6k.5 a
Can someone explain 6k.5 part a in the textbook? How is O3 to O2 a reduction if the oxidation numbers don't change? Both have a charge of 0.
- Thu Feb 29, 2024 8:54 pm
- Forum: Balancing Redox Reactions
- Topic: 6k.3 part d
- Replies: 1
- Views: 24
6k.3 part d
Can someone explain how to solve 6k.d 3 and why you solve it that way? Thanks
- Tue Feb 27, 2024 8:37 am
- Forum: Balancing Redox Reactions
- Topic: Oxidation numbers
- Replies: 1
- Views: 22
Oxidation numbers
Are there any oxidation numbers that we have to know from the periodic table? Or can we just know h and o?
- Tue Feb 27, 2024 8:36 am
- Forum: Balancing Redox Reactions
- Topic: H oxidation number
- Replies: 3
- Views: 50
H oxidation number
How can we tell if h has an oxidation number of negative one instead of positive one?
- Tue Feb 27, 2024 8:32 am
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: Nernst at 25 degrees
- Replies: 1
- Views: 42
Re: Nernst at 25 degrees
It’s not that the nernst equation is different at 25 degrees Celsius. We simply want to simplify the equation so we plug in a temperature. That way we get rid of a variable and can just use a constant for that given temperature. we could also plug in temperature to simplify the ln version.
- Tue Feb 27, 2024 8:28 am
- Forum: Balancing Redox Reactions
- Topic: oxidation numbers
- Replies: 1
- Views: 11
Re: oxidation numbers
H is plus one and O is negative 2
- Tue Feb 20, 2024 8:09 pm
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: Change in Entropy textbook problem example
- Replies: 1
- Views: 34
Re: Change in Entropy textbook problem example
To find entropy change at non transition temp:
Heat the substance to Boiling point (ΔS = ClnT2/T1)
Allow it to phase change ( ΔSvap = ΔHvap/TB)
Cool the vapor back down to temperature (ΔS = C lnT2/T1)
Heat the substance to Boiling point (ΔS = ClnT2/T1)
Allow it to phase change ( ΔSvap = ΔHvap/TB)
Cool the vapor back down to temperature (ΔS = C lnT2/T1)
- Tue Feb 20, 2024 8:01 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: q=c∆T
- Replies: 3
- Views: 76
Re: q=c∆T
For q of calorimeters we do not include moles. if calculating q of anything else (including the substance inside the calorimeter) we use q = nCT (or we can use grams).
- Tue Feb 20, 2024 7:59 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: j/mol vs j
- Replies: 2
- Views: 31
j/mol vs j
How do I know when to use j/mol as opposed to j when finding delta G or work?
- Tue Feb 20, 2024 11:23 am
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Textbook question 4.15 [ENDORSED]
- Replies: 1
- Views: 64
Textbook question 4.15 [ENDORSED]
Could someone explain how to find the enthalpy of the reaction in 4.15 of the book? The answer solution does something weird that doesn't follow our formula from class.
- Sun Feb 18, 2024 6:12 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: delta U = 3/2 n R delta T as opposed to delta U(m) = 3/2 R delta T
- Replies: 2
- Views: 24
delta U = 3/2 n R delta T as opposed to delta U(m) = 3/2 R delta T
When do we use delta U = 3/2 n R delta T as opposed to delta U(m) = 3/2 R delta T ? What are the uses and difference of these two equations?
- Sun Feb 18, 2024 6:11 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: delta U = 3/2 n R delta T
- Replies: 1
- Views: 24
delta U = 3/2 n R delta T
When do we use the equation delta U = 3/2 n R delta T?
- Sun Feb 18, 2024 6:10 pm
- Forum: Van't Hoff Equation
- Topic: vant hoff equation
- Replies: 1
- Views: 29
vant hoff equation
which form of the vant hoff equation do we need for the midterm?
- Sun Feb 18, 2024 6:09 pm
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: why does delta U equal zero during the isothermal expansion of an ideal gas?
- Replies: 2
- Views: 16
why does delta U equal zero during the isothermal expansion of an ideal gas?
Why does delta U equal zero during the isothermal expansion of an ideal gas? Or in a closed system?
- Sun Feb 18, 2024 6:07 pm
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: Systems
- Replies: 2
- Views: 11
Re: Systems
A living plant can exchange both energy and matter with its environment. Examples: it can take in solar energy and also take in gasses through its stomata
- Sun Feb 18, 2024 6:06 pm
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: Achieve Question #7
- Replies: 2
- Views: 36
Re: Achieve Question #7
Here are the steps you should take for this problem. First find delta H, then use delta H to find delta S. You find Delta H by finding the total number of joules added after the molecules get to their boiling point. You do this by multiplying 575 J/s by 60 s/min by 5.08 minutes (60 s/min was simply ...
- Sun Feb 18, 2024 6:04 pm
- Forum: Calculating Work of Expansion
- Topic: Irreversible or Reversible
- Replies: 2
- Views: 22
Re: Irreversible or Reversible
When to use irreversible:
Changing T
Constant Pexternal
expands/ compresses all at once
When to use reversible:
Isothermal (constant T)
Changing P
Reversible
Max work
Changing T
Constant Pexternal
expands/ compresses all at once
When to use reversible:
Isothermal (constant T)
Changing P
Reversible
Max work
- Sun Feb 18, 2024 6:02 pm
- Forum: Third Law of Thermodynamics (For a Unique Ground State (W=1): S -> 0 as T -> 0) and Calculations Using Boltzmann Equation for Entropy
- Topic: residual entropy
- Replies: 1
- Views: 16
Re: residual entropy
Molecules can have higher residual entropy as molecular complexity increases. This is because there are more possible bond vibrations that can absorb added energy. Also, if the molecule is symmetrical it will have a lower residual entropy compared to a similar molecule. The book BRIEFLY mentioned th...
- Sun Feb 18, 2024 5:58 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Achieve Question #7
- Replies: 1
- Views: 21
Re: Achieve Question #7
Hi! Here are the steps: First you're going to find delta H. Then, you'll find delta S. You find Delta H by finding the total number of joules added after the molecules get to their boiling point. This is done by multiplying 575 J/s by 60 s/min by 5.08 minutes. 60 s/min was simply your conversion fac...
- Sun Feb 18, 2024 5:55 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Achieve #18 Week3/4
- Replies: 1
- Views: 40
Re: Achieve #18 Week3/4
The definition of heat capacity is that C = q/(delta T). This is because heat capacity is measuring the change in temperature (delta T) associated with a transfer of heat (q). When we rearrange this equation we get q = C (delta T). Then, we scale up the equation by multiplying by mols because heat c...
- Sun Feb 18, 2024 5:47 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: achieve #18
- Replies: 5
- Views: 41
Re: achieve #18
It seems you haven't attached the problem! Maybe try submitting your question again.
- Sun Feb 18, 2024 5:46 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Achieve #7
- Replies: 2
- Views: 30
Re: Achieve #7
First you're going to find delta H, then find delta S. You find Delta H by finding the total number of joules added after the molecules get to their boiling point. You do this by multiplying 575 J/s by 60 s/min by 5.08 minutes (60 s/min was simply my conversion factor). This gives us 175260 Joules =...
- Sun Feb 18, 2024 5:40 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Calorimeter Application
- Replies: 1
- Views: 37
Re: Calorimeter Application
Hi! So calorimeters are special because they allow us to accurately measure the temperature change of a system in order to make deeper analyses of the system. The conditions of a system are adiabatic and closed, which is also known as isolated. So yes, it is essentially an isolated system that allow...
- Tue Feb 13, 2024 9:16 am
- Forum: Calculating Work of Expansion
- Topic: Sign of work
- Replies: 2
- Views: 46
Re: Sign of work
work is negative when the system is doing work. Work is positive when work is being done on the system
- Tue Feb 13, 2024 9:13 am
- Forum: Calculating Work of Expansion
- Topic: L*atm to J
- Replies: 1
- Views: 30
L*atm to J
How do you switch from L*atm to Joules?
- Sat Feb 10, 2024 4:13 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Delta H =q at constant pressure
- Replies: 2
- Views: 19
Delta H =q at constant pressure
Why does Delta H =q at constant presssure?
- Sat Feb 10, 2024 3:20 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Delta u = zero?
- Replies: 3
- Views: 56
Delta u = zero?
When does delta U equal zero? The textbook says that delta U equals zero for the isothermal compression or expansion of an ideal gas. Can someone please explain? What cases could we not use delta U equals zero? What are the implications?
- Tue Jan 30, 2024 7:17 pm
- Forum: Calculating Work of Expansion
- Topic: Reversible reactions vs irreversible reactions
- Replies: 1
- Views: 49
Re: Reversible reactions vs irreversible reactions
If a reaction is irreversible, it means that the acid or base is very strong and thus will completely ionize. Therefore, the concentration of the acid or base will be equal to the concentration of the conjugate acid or base. We can easily find the concentration of the ion or conjugate acid/base beca...
- Tue Jan 30, 2024 7:13 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Calculating calibration of caloriometer
- Replies: 1
- Views: 26
Re: Calculating calibration of caloriometer
If the specific heat capacity is given in Celcius, then the T should be in Celcius. Same for kelvin. Either works but you have to make sure they're coordinating.
- Tue Jan 30, 2024 7:10 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Percent ionization
- Replies: 5
- Views: 44
Percent ionization
Some different sources (achieve vs the textbook) have solved for percent ionization differently. Is percent ionization concentration of ion over initial concentration of acid or base? Or is the denominator the equilibrium concentration of the acid or base?
- Tue Jan 30, 2024 7:09 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: What changes K
- Replies: 1
- Views: 19
What changes K
Hi! What changes K? Is it only Temperature? Or can pressure change K too? If we change the pressure of the system by compressing the system, does the reaction shift or does the equilibrium concentration change?
- Tue Jan 23, 2024 11:39 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Important equations
- Replies: 2
- Views: 48
Important equations
What are the important equations to know for this chapter?
- Tue Jan 23, 2024 11:38 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Endothermic X2 <--> X
- Replies: 2
- Views: 36
Endothermic X2 <--> X
Question 5.33 in the book discusses that X2 <--> X is endothermic. How do we know this?
- Tue Jan 23, 2024 11:38 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Endothermic X2 <--> X
- Replies: 2
- Views: 44
Endothermic X2 <--> X
Question 5.33 in the book discusses that X2 <--> X is endothermic. How do we know this?
- Tue Jan 23, 2024 11:33 pm
- Forum: Phase Changes & Related Calculations
- Topic: Ionization percentages
- Replies: 2
- Views: 40
Re: Ionization percentages
Less than 5 percent means that it's okay to approximate (ignore the x in the denominator). This is just because this value corresponds with 10^-3 and is similarly negligable.
- Tue Jan 23, 2024 11:32 pm
- Forum: Calculating the pH of Salt Solutions
- Topic: Ka and Kb close to 10^-3
- Replies: 3
- Views: 52
Re: Ka and Kb close to 10^-3
He said that 10^-3 is the cutoff but for numbers that are very close we should operate our best judgement. Generally I'd rather be safe so I don't approximate. It's a bit more work but it should get you to the right answer.
- Tue Jan 23, 2024 11:29 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: pH
- Replies: 2
- Views: 32
Re: pH
A strong base will add OH- to the solution, so it will increase the pH. For instance, KOH is a strong base that will fully dissociate into K and OH, which will increase the concentration of OH and therefore decrease the pOH (pOH = -log [OH]). A smaller pOH means a higher pH.
- Tue Jan 23, 2024 11:23 pm
- Forum: Phase Changes & Related Calculations
- Topic: Acids and Bases
- Replies: 4
- Views: 62
Re: Acids and Bases
Bases will accept H+ or donate OH- and acids will donate H+. If you write a chemical reaction, look at what happens to the H+ or OH- concentration in water.
- Tue Jan 23, 2024 11:22 pm
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: weak/strong acid/base
- Replies: 3
- Views: 54
Re: weak/strong acid/base
Hi! So if it's a base, it's going to increase the OH- in the solution (so it'll either donate OH- or accept H+). If it's an acid, it'll donate H+ and increase the H+ concentration. You can tell if it's weak or strong in a few ways. First, weak bases/acids have low K values as they are not fully depr...
- Tue Jan 23, 2024 8:44 am
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: Achieve Question 5
- Replies: 1
- Views: 33
Re: Achieve Question 5
We would use pH = -log [h+] or convert to pOH and then find [ OH-]. This concentration is the concentration at equilibrium. Put this value over the initial concentration of the acid or base. Granted, you would need to be given the concentration of the acid or base initially.
- Tue Jan 16, 2024 8:42 am
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: What affects K?
- Replies: 2
- Views: 43
What affects K?
Which factors that we discussed will affect K? I know that K remains unchanged after some changes, and sometimes K can change. Which factors will change K and which will not?
- Tue Jan 16, 2024 8:33 am
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: le chateliers principle and pressure
- Replies: 3
- Views: 61
Re: le chateliers principle and pressure
Pressure does not affect liquids and solids so strongly. Liquids are pure substances and thus their concentrations remain the same despite change in pressure.
- Tue Jan 16, 2024 8:31 am
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: When can we ignore x
- Replies: 2
- Views: 45
When can we ignore x
There were some equations in class where we ignored the x on the bottom. When are we allowed to do this?
- Tue Jan 16, 2024 8:20 am
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Temperature Changes
- Replies: 1
- Views: 27
Re: Temperature Changes
For an endothermic reaction, increasing temperature will cause K to increase, and decreasing temperature will cause K to decrease. The same relationship is true for exothermic. Heating a reaction and cooling a system both have an affect on K for the reaction.
- Tue Jan 09, 2024 7:58 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Help explaining why a solid cannot be a concentration
- Replies: 5
- Views: 65
Re: Help explaining why a solid cannot be a concentration
Hi! A solid can not have a concentration as it is a pure substance!
- Tue Jan 09, 2024 7:57 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Balancing R and P
- Replies: 2
- Views: 22
Re: Balancing R and P
The conceptual reason why we have to balance the chemical reaction first is because the chemical reaction is showing how the molecules "switch off" in the reaction. For example, given the formula 2R --> 1P, balancing the formula is important because it shows that one mol of P is going to b...
- Tue Jan 09, 2024 7:51 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Is Ksp and Kc the same thing?
- Replies: 3
- Views: 59
Re: Is Ksp and Kc the same thing?
Additionally, you can calculate both Ksp and Kc using the same general formula, with the key exception that Ksp uses partial pressure and Kc uses concentration.
- Tue Jan 09, 2024 7:50 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Advice from a Medical Student [ENDORSED]
- Replies: 297
- Views: 494792
Re: Advice from a Medical Student [ENDORSED]
Thank you so much for sharing these tips!
- Tue Jan 09, 2024 7:21 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: 5G.3
- Replies: 5
- Views: 79
Re: 5G.3
We do not include solids or liquids in these calculations. This is because solids are pure substances and thus their concentration can not change. Liquids are not included because if a solute is in a liquid solvent, the solute is in such a negligible amount that the concentration is not changing sig...