Question

Analyzing a galvanic cell A galvanic cellis powered by the following redox reaction: NO3 (aq) + 4H' (aq) + 3 Cu+ (aq) → NO(g) + 2H2O(l) + 3 Cu2+(aq)

Answer the following questions about this cell.
If you need any electrochemical data, be sure you
Write a balanced equation for the half-reaction that takes place at the cathode.
Write a balanced equation for the half-reaction that takes place at the anode.
Calculate the cell voltage under standard conditions Round your answer to 2 decimal places.

Answer 1

The cathode half-reaction for the given galvanic cell involves the reduction of nitrate to nitric oxide, while the anode half-reaction involves the oxidation of copper(I) to copper(II). To calculate the cell voltage under standard conditions, standard reduction potentials for each half-reaction are needed which are not provided in this case.

Step-by-step explanation:

The given galvanic cell is powered by the redox reaction: NO3- (aq) + 4H+ (aq) + 3 Cu+ (aq) → NO(g) + 2H2O(l) + 3 Cu2+(aq).

The cathode half-reaction involves reduction and for the given reaction, it would be:

NO3- (aq) + 4H+ (aq) + 3e- → NO(g) + 2H2O(l) (reduction of nitrate to nitric oxide)

The anode half-reaction involves oxidation and is represented by:

3 Cu+ (aq) - 3e- → 3 Cu2+ (aq) (oxidation of copper(I) to copper(II))

To calculate the cell voltage under standard conditions, you would use the standard reduction potentials for each half-reaction, found in a standard reduction potential table. The cell voltage (Ecell) is calculated by subtracting the anode potential from the cathode potential (Ecell = Ecathode - Eanode). Since the exact standard reduction potentials are not provided here, we cannot calculate the cell voltage.