Search found 31 matches
- Sat Mar 16, 2019 8:16 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: 4c.3
- Replies: 1
- Views: 412
Re: 4c.3
There is no change in enthalpy for part b since it is under constant volume, not pressure. You would use 765 J= qv
- Sat Mar 16, 2019 8:09 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: Question 14.51
- Replies: 1
- Views: 436
Re: Question 14.51
For this problem, you solve for Ecell, using this formula for the Nernst equation: Ecell=Eocell-(0.025693V/n)lnQ. Then substitute that value in for deltaG= -nFEcell.
- Sat Mar 16, 2019 8:00 pm
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: Determining n
- Replies: 6
- Views: 843
Re: Determining n
The easiest way to figure out n is to split the the reaction into its reducing and oxidizing half-reactions, and then balance out those reactions os they both have the same number of e- in each rxn. For part b), we know to put the 14H+ for Cr because we see that its product has an O in it, meaning t...
- Sun Mar 10, 2019 7:21 pm
- Forum: First Order Reactions
- Topic: 7B.9a
- Replies: 1
- Views: 263
7B.9a
Could someone please help me on part a? Thanks!
For the first-order reaction A-->3B + C when [A]0=0.015 mol.L^-1, the concentration of B increases to 0.018 mol.L^-1 in 3.0 min
a) What is the rate constant for the reaction expressed at the rate of loss of A?
For the first-order reaction A-->3B + C when [A]0=0.015 mol.L^-1, the concentration of B increases to 0.018 mol.L^-1 in 3.0 min
a) What is the rate constant for the reaction expressed at the rate of loss of A?
- Sun Mar 10, 2019 7:11 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Final Exam
- Replies: 23
- Views: 1848
Re: Final Exam
Yes, I believe the final is cumulative, so chemical equilibria will probably be on the exam.
It is under the file titled "Important Final Exam Information" on the 14B website I think :)
It is under the file titled "Important Final Exam Information" on the 14B website I think :)
- Sun Mar 10, 2019 7:03 pm
- Forum: Second Order Reactions
- Topic: 7B.13 Help
- Replies: 4
- Views: 500
7B.13 Help
Could someone help to explain this question to me?
Q:The half-life of A in a second-order reaction is 50.5s when [A]0= 0.84 mol. L^-1. Calculate the time needed for the concentration of A to decrease to
a) one-sixteenth
b) one-fourth
c) one-fifth
Thank you!
Q:The half-life of A in a second-order reaction is 50.5s when [A]0= 0.84 mol. L^-1. Calculate the time needed for the concentration of A to decrease to
a) one-sixteenth
b) one-fourth
c) one-fifth
Thank you!
- Thu Feb 28, 2019 10:49 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: 6M.1
- Replies: 1
- Views: 356
6M.1
A student was given a standard Cu(s)|Cu2+ (aq) half-cell and another half-cell containing an unknown metal M in 1.00 M M(NO3)2(aq) and formed the cell M(s)|M+(aq)||Cu2+ (aq)|Cu(s). The cell potential was found to be -0.689 V. What is the value of E(M2+/M)? From the cell diagram, I though Cu/Cu2+ was...
- Thu Feb 28, 2019 10:39 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: 6L.9
- Replies: 1
- Views: 228
6L.9
a) Write balanced half-reactions for the redox reaction of an acidified solution of potassium permanganate and iron(II) chloride. b) Write the balanced equation for the cell reaction and devise a galvanic cell to study the reaction (write its cell diagram) For this reaction, how do you determine whi...
- Thu Feb 28, 2019 10:13 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: 6L.7a Help
- Replies: 1
- Views: 289
6L.7a Help
Write the half-reactions and devise a galvanic cell (write a cell diagram) to study each of the following reactions:
a) AgBr(s)--> Ag+ (aq) + Br-(aq), a solubility equilibrium
Could someone explain to me how to approach this problem? Thanks!
a) AgBr(s)--> Ag+ (aq) + Br-(aq), a solubility equilibrium
Could someone explain to me how to approach this problem? Thanks!
- Mon Feb 25, 2019 12:56 pm
- Forum: Balancing Redox Reactions
- Topic: Balancing Redox Reactions in Basic Solutions
- Replies: 1
- Views: 234
Re: Balancing Redox Reactions in Basic Solutions
Essentially, the methods are the same as the acidic reaction up until the part when you have to cancel out electrons. From that point, you add an additional step where you add the same amount of OH- ions on both sides so that the number of H+ ions will completely react with the OH- ions to create H2...
- Mon Feb 25, 2019 12:51 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Platinum in Cell Diagrams
- Replies: 1
- Views: 224
Platinum in Cell Diagrams
If one side of the diagram yields no solid metal, do we automatically know that we should write Pt(s) on that side? Is there a way to know which alternative metal we use, if we don't use Pt(s)?
- Mon Feb 25, 2019 12:44 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Cell Potential Value
- Replies: 1
- Views: 424
Cell Potential Value
Just for clarification from Friday's lecture, why does the E of a reduction/oxidation reaction not change whenever you alter a reaction by multiplying the coefficients? Thanks in advance!
- Sun Feb 17, 2019 10:09 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Problem 115 ch 11 6th edition
- Replies: 2
- Views: 278
Re: Problem 115 ch 11 6th edition
In this case, we consider Le Chatelier's Principle. If the partial pressure of O2 were to increase, there would be more O2 molecules present, which results in the equilibrium ratio having a higher partial pressure of O2 than initially (Qp>Kp). To minimize this effect, the reaction will shift to the ...
- Sun Feb 17, 2019 9:43 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Elements with Gibbs Free Energy
- Replies: 1
- Views: 234
Elements with Gibbs Free Energy
Do all elements in their most stable form have standard Gibbs Free Energy of formation of zero? If so, could someone conceptually explain to me why this is so?
- Sun Feb 17, 2019 9:36 pm
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: Entropy with Temperature and Volume
- Replies: 2
- Views: 1467
Re: Entropy with Temperature and Volume
For those particular problems, you need to solve for a total change in entropy caused by both temperature and volume. I believe in those cases we are generally considering a reversible reaction, so we use two separate equations, one for temperature change (S=nCln(T2/T1)) and another for volume (S=nR...
- Sun Feb 10, 2019 4:07 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: Entropy at Equilibrium
- Replies: 1
- Views: 217
Entropy at Equilibrium
Could someone re-explain for me why entropy is a maximum at equilibrium? More specifically, could someone explain why at equilibrium, all possible states have been reached?
- Sun Feb 10, 2019 4:03 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: 11.89 6th edition
- Replies: 1
- Views: 235
Re: 11.89 6th edition
Yes, I believe that is the case because they're converting it to atm I think.
- Sun Feb 10, 2019 4:02 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: HW Prolem (4G.4) 7th Edition
- Replies: 2
- Views: 251
Re: HW Prolem (4G.4) 7th Edition
COF2 would have a higher molar entropy than BF3. When you take a look at the molecular structures, BF3 is a trigonal planar with the same B-F bond on each end. This means that is it very ordered, compared to COF2, which has two F's and an O at the ends. This means that for some molecules, it could p...
- Sun Feb 03, 2019 1:48 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: 8.101b 6th edition
- Replies: 1
- Views: 150
Re: 8.101b 6th edition
SO2 would be the limiting reactant because if you had 0.030 mol of O2, then by the molar ratio given to us by the coefficients of the reaction (2 mol SO2 for every 1 mol of O2), then you'd need 0.060 mol of SO2 to fully react. However, in the question, we are given only 0.030 mol of SO2, half the nu...
- Sun Feb 03, 2019 1:44 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: 103 6th edition
- Replies: 2
- Views: 276
Re: 103 6th edition
I believe average kinetic energy is calculated using the formula 3/2RT
- Sun Feb 03, 2019 1:30 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Why Bond Enthalpies are the least accurate
- Replies: 3
- Views: 1758
Re: Why Bond Enthalpies are the least accurate
Bond enthalpy is the least accurate because it represents the average of a series of different bonds from different molecules, so it represents an approximation of a bond rather than a more precise measurement like formation.
Hope that helps!
Hope that helps!
- Sun Feb 03, 2019 1:27 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Seventh Edition ? 4C.3
- Replies: 1
- Views: 230
Re: Seventh Edition ? 4C.3
To approach this problem, you'd first have to recognize that you're using the formula qp=nCp,mdeltaT. You would then substitute given values, with 765 J being qp, 0.820 mol for n, and 298 K for initial temperature. However, in this problem, you'd also have to recognize the rotational contribution of...
- Sat Jan 26, 2019 10:54 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Method 2 Example
- Replies: 3
- Views: 243
Method 2 Example
On Friday's Lecture, there was an example for Method 2 which considered the bond enthalpies regarding CH2=CH2 + H-Br --> CH3-CH2Br Could someone reiterate why we utilized the value of the C=C bond on the reactants' side, and why we considered using the bond enthalpy of C-C on the products' side? I g...
- Sat Jan 26, 2019 10:30 pm
- Forum: Phase Changes & Related Calculations
- Topic: 6th edition 8.15
- Replies: 1
- Views: 887
Re: 6th edition 8.15
Hello, I hope these answers help! a) The change in internal energy would only be zero if q+w=0. Since we've established no energy is transferred as heat (q=0) we can then say that this statement is only true when w=0, or if no work is done b) This is always true because the question stated that ther...
- Thu Jan 24, 2019 2:30 pm
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: 6B.9
- Replies: 1
- Views: 610
6B.9
6B.9 a) Complete the following table [H3O+] [OH-] pH pOH i) 1.50 mol.L-1 ii) 1.50 mol.L-1 iii) 0.75 iv) 0.75 b) Rank the four solutions in order of increasing acidity (I understand iii) and iv), but I am not sure why I keep getting i) and ii) wrong. When I calculate for i), I get [OH-]= 6.67x10^-15 ...
- Mon Jan 21, 2019 10:08 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Chemical Equilibrium part 4 post module assessment question #12
- Replies: 2
- Views: 263
Re: Chemical Equilibrium part 4 post module assessment question #12
Both sides of the reaction contain the same number of moles (2:2), so the reaction doesn't favor any particular side.
- Mon Jan 21, 2019 9:49 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Approximating for Equilibrium Constants
- Replies: 1
- Views: 143
Re: Approximating for Equilibrium Constants
Hey there! I believe we could use this method with Kc as well, if we needed it.
- Mon Jan 21, 2019 9:47 pm
- Forum: Identifying Acidic & Basic Salts
- Topic: Effect of pH
- Replies: 2
- Views: 405
Effect of pH
Hello there, not sure if anyone asked this already, but could someone explain to me how we know that Group I/II and some of the halogens (Cl-, Br-. I-) have no effect on the pH when it dissociates in water?
- Fri Jan 11, 2019 7:46 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Changes in Systems
- Replies: 3
- Views: 324
Re: Changes in Systems
I believe that this is always the case. There is an equation relating the temperature to K that may help you understand why, and you can see the full derivation of it in the textbook (For me, it is in 5H, pg 413, not sure about the 6th edition)
Hop this helps
Hop this helps
- Fri Jan 11, 2019 7:36 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Q 11.49
- Replies: 1
- Views: 86
Re: Q 11.49
Hey there! I believe it has to do with the coefficient of the reactant, which has a 2 on it, I assume (Sorry, I'm not too sure about this because I don't think I have the same edition as you) If there's a 2 as a coefficient, we have to consider this when forming the ICE Box. In this case, if the pro...
- Fri Jan 11, 2019 7:28 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: 6th edition 11.71
- Replies: 1
- Views: 467
Re: 6th edition 11.71
Not sure if you wanted all of the answers, but I provided them all down below with some explanations. Hope it helps! a) When you add NO, Q>K, so more reactants are formed. This means more products are used up, so the amount of H2O, which we assume is constant and hasn't changed in concentration, dec...