Question

Enter electrons as e^-.

Use smallest possible integer coefficients.

If a box is not needed, leave it blank.

A voltaic cell is constructed from a standard Mn²⁺|Mn half cell (E°_red = -1.180V) and a standard Cu²⁺|Cu⁺ half cell (E°_red = 0.153V).  

The anode reaction is:

The cathode reaction is:

The spontaneous cell reaction is:

The cell voltage is _____ V.

Answer 1

for the given cell,

The half reactions are,

Mn+2 + 2e- ------> Mn ; E0 red = -1.180V

Cu+2 + e- -----> Cu+ ; E0 red = 0.153V

The half cell which has lower E0 red value undergo oxidation and another one undergo reduction process,

so the anode half reaction (oxidation half reaction),

Mn -----> Mn+2 + 2e- ; E0 red = -1.180V

the cathode half reaction ( reduction half reaction),

Cu+2 + e- ----> Cu+ ; E0 red = +0.153V

The spontaneous cell reaction,

2Cu+2 + Mn ------> Mn+2 + 2Cu+ ; E0 cell = (E0 red) of cathode - (E0 red) of anode

E0 cell or cell voltage = 0.153 - (-1.180) = 1.333V