Question

Given that E o = 0.52 V for the reduction Cu+(aq) + e− → Cu(s), calculate...

Given that E o = 0.52 V for the reduction Cu+(aq) + e− → Cu(s), calculate E o , ΔG o , and K for the following reaction at 25°C: 2Cu+(aq) ⇌ Cu2+(aq) + Cu(s)

E o = V

ΔG o = kJ

K = × 10

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
For the following reactions and given standard reduction potentials O2(g) + 4H+(aq) + 2Cu(s)  2Cu2+(aq)...
For the following reactions and given standard reduction potentials O2(g) + 4H+(aq) + 2Cu(s)  2Cu2+(aq) + 2H2O(l) O2(g) + 4H+(aq) + 4e-  2H2O(l)       E° = 1.23 V Cu2+ + 2e-  Cu(s)    E° = 0.34 V a. Calculate E°cell b. Calculate ΔG° at 254 K
Given the cell reaction : 2 Cl – (aq) + Cu2+(aq)→ Cl2 (aq) + Cu (s)...
Given the cell reaction : 2 Cl – (aq) + Cu2+(aq)→ Cl2 (aq) + Cu (s) a) As written, is the cell galvanic or electrolytic? b) Calculate E°cell. c) Calculate ΔG°. 3. Using the standard reduction potentials given in Appendix of your text book, calculate the cell potential (E°cell ) at 298 K for each of the following reactions. (A) Br2 (aq) + 2 ClV (aq) → 2BrV (aq) + Cl2 (g) (B) A Galvanic Cell with the SHE and...
Use the standard reduction potentials shown here to answer the questions. Reduction half-reaction E∘ (V) Cu2+(aq)+2e−→Cu(s)...
Use the standard reduction potentials shown here to answer the questions. Reduction half-reaction E∘ (V) Cu2+(aq)+2e−→Cu(s) 0.337 2H+(aq)+2e−→H2(g) 0.000 A copper, Cu(s), electrode is immersed in a solution that is 1.00 M in ammonia, NH3, and 1.00 M in tetraamminecopper(II), [Cu(NH3)4]2+. If a standard hydrogen electrode is used as the cathode, the cell potential, Ecell, is found to be 0.073 V at 298 K. Part A Based on the cell potential, what is the concentration of Cu2+ in this solution?...
4a. Use the Nernst equation to calculate the cell voltage (E) for the following redox reaction:...
4a. Use the Nernst equation to calculate the cell voltage (E) for the following redox reaction: i. Fe3+(aq)+Cu(s)→Cu2+(aq)+Fe2+(aq), given that [Fe3+]=0.05 and [[Cu2+]=0.125M at 25°C, and Fe3++e→Fe2+             E0=0.77 V Cu2+2e→Cu                   E0=0.34 V 4b. Use the information provided in question 4a to calculate the change in free energy (ΔG) and change in entropy (ΔS) for the redox reaction: i. Fe3+(aq)+Cu(s)→Cu2+(aq)+Fe2+(aq) What do the ΔG and ΔS values indicate about the spontaneity of the redox reaction?
7. Determine Eo for the following reaction, using the given standard reduction potentials: Cu(s) + Fe2+(aq)...
7. Determine Eo for the following reaction, using the given standard reduction potentials: Cu(s) + Fe2+(aq) → Cu+(aq) + Fe(s) Eo for Fe2+(aq) = -0.44 V Eo for Cu+(aq) = 0.52 V 8. Consider the following half-reactions. Which of these is the strongest oxidizing agent listed here? I2(s) + 2 e- → 2 I-(aq) Eo = 0.53 V S2O82-(aq) + 2 e- → 2 SO42-(aq) Eo = 2.01 V Cr2O72-(aq) + 14 H+ + 6 e- → Cr3+(aq) + 7...
Constants The following values may be useful when solving this tutorial. Constant Value E∘Cu 0.337 V...
Constants The following values may be useful when solving this tutorial. Constant Value E∘Cu 0.337 V E∘Ni -0.257 V R 8.314 J⋅mol−1⋅K−1 F 96,485 C/mol T 298 K Part A In the activity, click on the E∘cell and Keq quantities to observe how they are related. Use this relation to calculate Keq for the following redox reaction that occurs in an electrochemical cell having two electrodes: a cathode and an anode. The two half-reactions that occur in the cell are...
Calculate ?cell for the following concentration cell ? Cu(s) | Cu2+ (aq, 0.025M) ? Cu2+ (aq,...
Calculate ?cell for the following concentration cell ? Cu(s) | Cu2+ (aq, 0.025M) ? Cu2+ (aq, 0.30M) | Cu(s) Cu2+ (aq) + 2e- ? Cu(s) ? ?° = 0.340V A)0.0638 V B)-0.0734 V C)0.0734 V D)-0.0319 V E)0.0139 V
Consider the half reactions below. Cu 2+ (aq) + 2 e- -----> Cu (s) Eo =...
Consider the half reactions below. Cu 2+ (aq) + 2 e- -----> Cu (s) Eo = 0.34 V MnO4 - (aq) + 4 H+ (aq) + 3 e- -----> MnO2 (s) + 2 H2O (l) Eo = 1.68 V A. What is the standard cell potential for a voltaic cell comprised of these two half reactions? B. What is the equilibrium constant for this reaction at 25 oC? C. How is the magnitude of the equilibrium constant consistent with a...
Au3+(aq) + 3e- --> Au(s) 1.498 V Ag+(aq) + e- --> Ag(s) 0.767 V Cu2+(aq) +...
Au3+(aq) + 3e- --> Au(s) 1.498 V Ag+(aq) + e- --> Ag(s) 0.767 V Cu2+(aq) + 2e- --> Cu(s) 0.342 V Ni2+(aq) + 2e- -->Ni(s) -0.257 V Calculate the potential at 25ºC for the following cell: Cu | Cu2+ [0.024M] || Ag+ [0.0048M] | Ag
1. A constant electric current flows for 3.35 h through electrolytic cells connected in series. One...
1. A constant electric current flows for 3.35 h through electrolytic cells connected in series. One contains a solution of AgNO3, and the second contains a solution of CuCl2. During this time, 1.80 g of silver is deposited in the first cell. (a) How many grams of copper are deposited in the second cell? g Cu (b) What is the current flowing in (in amperes) ?   A 2. Oxalic acid (H2C2O4) is present in many plants and vegetables. (a) Balance...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT