Problem: A chemist designs a galvanic cell that uses these two half-reactions:Half-reaction standard reduction potentialMnO4- (aq) + 8H+ (aq) + 5e- → Mn2+ (aq) + 4H2O (l) E°red = + 1.51 VFe3+ (aq) + e- → Fe2+ (aq) E°red = +0.771 VAnswer the followingWrite a balanced equation for the half-reaction that happens at the cathode.Write a balanced equation for the half-reaction that happens at the anode.Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. Do you have enough information to calculate the cell voltage under standard conditions?a) yesb) noIf you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your answer to 2 significant digits.
FREE Expert Solution
Write a balanced equation for the half-reaction that happens at the cathode.
• ↑ E° → reduction → cathode
Cathode: MnO4- (aq) + 8H+ (aq) + 5e- → Mn2+ (aq) + 4 H2O (l) E°red = + 1.51 V
Write a balanced equation for the half-reaction that happens at the anode.
• ↓ E° → oxidation → anode
Anode: Fe3+ (aq) + e- → Fe2+ (aq) E°red = +0.771 V
Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.
Problem Details
A chemist designs a galvanic cell that uses these two half-reactions:
Half-reaction standard reduction potential
MnO4- (aq) + 8H+ (aq) + 5e- → Mn2+ (aq) + 4H2O (l) E°red = + 1.51 V
Fe3+ (aq) + e- → Fe2+ (aq) E°red = +0.771 V
Answer the following
Write a balanced equation for the half-reaction that happens at the cathode.
Write a balanced equation for the half-reaction that happens at the anode.
Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.
Do you have enough information to calculate the cell voltage under standard conditions?
a) yes
b) no
If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your answer to 2 significant digits.