The standard reduction potentials at 295 K for the following half cells are given below:
+ 4H + + 3e - 
NO(g)+2H 2 O E° = 0.97 V
V 2+ (aq)+2e - 
V(s) E° = -1.19 V
Fe 3+ (aq)+3e - 
Fe(s) E° = -0. 04 V
A g + (aq)+e - 
Ag(s) E° = 0.80 V
Au 3+ (aq)+3e - 
Au(s) E° = 1. 40 V
The number of metal(s) which will be oxidised by 
in aqueous solution is_____.
Text Solution
Verified by Experts3
(3) For feasibility, check, E° cell = E° cathode(reduction) - E° anode(oxidation) > 0
The E° values when metal acts as anode and 
reaction is cathodic reaction.
For Vanadium metal, E° cell = 0.97 + 1.19 = 2.16V
For Iron metal, E° cell = 0. 97 + 0. 04 = 1. 01V
For silver metal, E° cell = 0.97 - 0.80 = 0.17V
For Gold metal, E° cell = 0.97 - 1.140 = -0.17V
For electrodes having oxidation potential greater than -0.97 V, E° cell > 0
Ag, Fe and V can be oxidised
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