Question

What is the standard cell potential for an electrochemical cell based on the following half-reactions? IO3-(aq)...

What is the standard cell potential for an electrochemical cell based on the following half-reactions?

IO3-(aq) + 6 H+(aq) + 6 e- ----> I-(aq) + 3 H2O(l ) E° = 1.085 V

Zn2+(aq) + 2 e- ---> Zn(s) E° = -0.762 V

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

Given,

IO3-(aq) + 6 H+(aq) + 6 e- ----> I-(aq) + 3 H2O(l ) E° = 1.085 V

3 Zn2+(aq) + 6 e- ---> 3 Zn(s) E° = -0.762 V

=> 3 Zn -------> 3 Zn2+ + 6 e-                                                        E° = 0.762 V

Overall reaction :

3 Zn + IO3- + 6H+ -----> 3 Zn2+ + I- + 3H2O

Eo = 1.085 V + 0.762 V = 1.847 V = Standard cell potential

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
Short Answer 1) Reduction half-reactions with corresponding standard half-cell potentials are shown below. Zn2+(aq) + 2...
Short Answer 1) Reduction half-reactions with corresponding standard half-cell potentials are shown below. Zn2+(aq) + 2 e‐ → Zn(s) E° = ‐ 0.76 V Al3+(aq) + 3 e‐ → Al(s) E° = ‐ 1.66 V The standard potential for the galvanic cell that uses these two half-reactions is ________ V. 2)In the galvanic cell represented by the shorthand notation shown below, Cd(aq)|Cd2+(aq)|| I2(g)|I-(aq)|Pt(s) the inert electrode is ________, and the balanced cathode half-reaction reaction is ________.
Assume you are constructing a Galvanic cell based on the half-reactions between Zn2+(aq)/Zn(s) and Ag+(aq)/Ag. The...
Assume you are constructing a Galvanic cell based on the half-reactions between Zn2+(aq)/Zn(s) and Ag+(aq)/Ag. The standard reduction potentials are given below. Ag+ (aq) + e- Ag (s) Eo = 0.80 V Zn2+ (aq) + 2 e- Zn(s) Eo = -0.76 V Write a balanced chemical REDOX equation and determine the Eo for the cell. What will be observed at the cathode and at the anode? Is the reaction thermodynamically favored? Explain.
Calculate the cell potential for the voltaic cell based on the following half reactions at T...
Calculate the cell potential for the voltaic cell based on the following half reactions at T = 25ºC: Cr3+(aq) + 3e- → Cr(s) Eº = - 0.74 V TiO2+(aq) + 2H+ (aq) + 1e- → Ti3+(aq) + H2O(l) Eº = + 0.10 V Where, [Cr3+] = 1.0 x 10-4 M, [TiO2+] = 1.0 x 10-1 M, [H+] = 1.0 M, [Ti3+] = 5.0 x 10-2 M.
An electrochemical cell is based on the following two half-reactions: Ox: Sn(s)→Sn2+(aq, 1.50 M )+2e− Red:...
An electrochemical cell is based on the following two half-reactions: Ox: Sn(s)→Sn2+(aq, 1.50 M )+2e− Red: ClO2(g, 0.150 atm )+e−→ClO−2(aq, 1.50 M ) Compute the cell potential at 25 ∘C .
What is the calculated value of the cell potential at 298 K for an electrochemical cell...
What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the H2 pressure is 5.00×10-3 bar, the H+ concentration is 1.46 M, and the Zn2+concentration is 3.42×10-4 M ? 2H+(aq) + Zn(s) ----> H2(g) + Zn2+(aq) Answer: _____ V ? The cell reaction as written above is product-favored (spontaneous) for the concentrations given: _______(true/false)?
An electrochemical cell is based on the following two half-reactions: Ox: Sn(s)?Sn2+(aq, 1.60 M )+2e? Red:...
An electrochemical cell is based on the following two half-reactions: Ox: Sn(s)?Sn2+(aq, 1.60 M )+2e? Red: ClO2(g, 0.195 atm )+e??ClO?2(aq, 1.70 M ). Compute the cell potential at 25 degrees C.
Reduction half-reactions with corresponding standard half-cell potentials are shown below. Zn2+(aq) + 2 e- ? Zn(s)...
Reduction half-reactions with corresponding standard half-cell potentials are shown below. Zn2+(aq) + 2 e- ? Zn(s) E
An electrochemical cell is based on the following two half-reactions: Ox: Pb(s)→Pb2+(aq, 0.11 M )+2e− Red:...
An electrochemical cell is based on the following two half-reactions: Ox: Pb(s)→Pb2+(aq, 0.11 M )+2e− Red: MnO−4(aq, 1.70 M )+4H+(aq, 2.6 M )+3e−→ MnO2(s)+2H2O(l) Part A Compute the cell potential at 25 ∘C. Please show all work. Thank you.
Constants | Periodic Table An electrochemical cell is based on the following two half-reactions: oxidation: Sn(s)→Sn2+(aq,...
Constants | Periodic Table An electrochemical cell is based on the following two half-reactions: oxidation: Sn(s)→Sn2+(aq, 2.00 M )+2e− reduction: ClO2(g, 0.290 atm )+e−→ClO−2(aq, 1.65 M ) You may want to reference (Pages 865 - 869) Section 19.6 while completing this problem. Part A Compute the cell potential at 25 ∘C. Express the cell potential to three significant figures.
A galvanic cell is based on the following half-reactions at 281 K: Cu+ + e- →...
A galvanic cell is based on the following half-reactions at 281 K: Cu+ + e- → Cu     Eo = 0.521 V H2O2 (aq) + 2 H+ + 2 e- → 2 H2O     Eo = 1.78 V What will the potential of this cell be when [Cu+] = 0.567 M, [H+] = 0.00333 M, and [H2O2] = 0.861 M? Enon
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT