Write the overall chemical reaction and calculate E° for the following reduction and oxidation half-reactions.
2H⁺(aq) + 2e? ? H₂(g) ${E}_{\text {red }}^{0}$ = 0.000 V
Zn(s) ? Zn²⁺(aq) + 2e? $E_{o x}^{\circ}$ = +0.762 V

Question

Write the overall chemical reaction and calculate E° for the following reduction and oxidation half-reactions.
2H⁺(aq) + 2e? ? H₂(g)

{E}_{\text {red }}^{0}

= 0.000 V
Zn(s) ? Zn²⁺(aq) + 2e?

E_{o x}^{\circ}

= +0.762 V

Quizplus · Accepted Answer

To determine the overall reaction, we need to add the reduction and oxidation half-reactions:
2HS1U1P1+S1S1P0(aq)+ 2e− → HS1U1B12S1U1B0(g) E° = 0.000 V (reduction half-reaction)
Zn(s)→ ZnS1U1P12+S1S1P0(aq)+ 2e− E° = +0.762 V (oxidation half-reaction)

If we reverse the reduction half-reaction, we get:
HS1U1B12S1U1B0(g) → 2HS1U1P1+S1S1P0(aq)+ 2e− E° = 0.000 V

Now we can add these reactions together, cancelling out the electrons:
Zn(s) + HS1U1B12S1U1B0(g) → ZnS1U1P12 + 2HS1U1P1+S1S1P0(aq) E° = +0.762 V (overall reaction)

Therefore, the best choice is C, which is the same as the overall reaction we derived.

Write the Overall Chemical Reaction and Calculate E° for the Following