# Problem: What is the E°cell for the cell represented by the combination of the following half-reactions?2Hg2+(aq) + 2e– ⇌ Hg22+(aq)               E° = 0.92 VCr3+ (aq) + 3e– ⇌ Cr(s)                            E° = –0.74 VA) –0.18 VB) 0.18 VC) 1.28 VD) 1.66 VE) 2.12 V

###### FREE Expert Solution

We’re being asked to determine the standard cell potential (E°cell) for the cell represented by the combination of the following half-reactions:

2 Hg2+(aq) + 2 e ⇌ Hg22+(aq)               E° = 0.92 V
Cr3+ (aq) + 3 e ⇌ Cr(s)                         E°= –0.74 V

To calculate for the standard cell potential, use the following equation:

$\overline{){\mathbf{E}}{{\mathbf{°}}}_{{\mathbf{cell}}}{\mathbf{=}}{\mathbf{E}}{{\mathbf{°}}}_{{\mathbf{cathode}}}{\mathbf{-}}{\mathbf{E}}{{\mathbf{°}}}_{{\mathbf{anode}}}}$

We can determine the anode and cathode by comparing their E° values. ###### Problem Details

What is the E°cell for the cell represented by the combination of the following half-reactions?

2Hg2+(aq) + 2e ⇌ Hg22+(aq)               E° = 0.92 V

Cr3+ (aq) + 3e ⇌ Cr(s)                            E° = –0.74 V

A) –0.18 V

B) 0.18 V

C) 1.28 V

D) 1.66 V

E) 2.12 V