# 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.

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###### 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

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Cell Potential concept. If you need more Cell Potential practice, you can also practice Cell Potential practice problems.