Calculate the e.m.f. of the cell,
Mg/Mg2+ (0.1 M) || Ag+ (1.0 x 10^3 M)/Ag
The values of E Mg2+ /Mg
and E
2.37 V and + 0.80 V respectively.
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Given:
Mg/Mg2+ (0.1 M) || Ag+ (1.0 x 10^3 M)/Ag. The values of E Mg2+ /Mg and E 2.37 V and + 0.80 V respectively
To find:
Calculate the e.m.f. of the cell
Solution:
From given, we have,
Mg/Mg2+ (0.1 M) || Ag+ (1.0 x 10^3 M)/Ag.
The values of E Mg2+ /Mg and E - 2.37 V and + 0.80 V respectively
The emf of the cell is given by the formula,
E° cell = E° cathode - E° anode
From given, we have,
E° cathode = 0.80 V
E° anode = - 2.37 V
thus substituting the given values in the above equation, we get,
E° cell = 0.80 - (- 2.37)
= 0.80 + 2.37
∴ The e.m.f. of the cell, E° cell = 3.17 V
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