# Problem: Consider the following half-reactions and their standard reduction potentials then give the standard line (cell) notation for a voltaic cell built on these half reactions.Mn2+ (aq) + 2 e- ⇌ Mn(s)                   E° = -1.18 VCr3+ (aq) + 3 e-⇌ Cr(s)                      E° = -0.41 Va. Mn (s) | Mn2+(aq, 1.0 M) || Cr3+(aq, 1.0 M) | Cr(s)b. Mn2+(aq, 1.0 M) | Mn (s) || Cr3+(aq, 1.0 M) | Cr(s)c. Mn2+(aq, 1.0 M) | Mn (s) || Cr3+(aq, 1.0 M)d. Cr(s) l Cr3+(aq, 1.0 M) || Mn (s) | Mn2+(aq, 1.0 M)e. Cr3+(aq, 1.0 M) l Cr(s) ll Mn2+(aq, 1.0 M) | Mn (s)

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###### FREE Expert Solution

We’re being asked to determine the cell notation for the redox reaction shown below:

Mn2+ (aq) + 2 e- ⇌ Mn(s)                   E° = -1.18 V

Cr3+ (aq) + 3 e-⇌ Cr(s)                      E° = -0.41 V

When writing a cell notation, we use the following format – “as easy as ABC To determine the cell notation of the reaction, we will use the following steps:
Step 1: Determine the anode and the cathode.
Step 2Write the cell notation of the reaction. ###### Problem Details

Consider the following half-reactions and their standard reduction potentials then give the standard line (cell) notation for a voltaic cell built on these half reactions.

Mn2+ (aq) + 2 e- ⇌ Mn(s)                   E° = -1.18 V

Cr3+ (aq) + 3 e-⇌ Cr(s)                      E° = -0.41 V

a. Mn (s) | Mn2+(aq, 1.0 M) || Cr3+(aq, 1.0 M) | Cr(s)

b. Mn2+(aq, 1.0 M) | Mn (s) || Cr3+(aq, 1.0 M) | Cr(s)

c. Mn2+(aq, 1.0 M) | Mn (s) || Cr3+(aq, 1.0 M)

d. Cr(s) l Cr3+(aq, 1.0 M) || Mn (s) | Mn2+(aq, 1.0 M)

e. Cr3+(aq, 1.0 M) l Cr(s) ll Mn2+(aq, 1.0 M) | Mn (s)