Calculatethe standard cell potentials of galvanic cells in which the followingreactions take place:

(i) 2Cr(s) + 3Cd2+(aq)→ 2Cr3+(aq)+ 3Cd

(ii) Fe2+(aq)+ Ag+(aq)→ Fe3+(aq)+ Ag(s)

Calculatethe Δr G θand equilibrium constant of the reactions.

(i)

Thegalvanic cell of the given reaction is depicted as:

Now,the standard cell potential is

Inthe given equation,

n= 6

F =96487 C mol−1

= +0.34 V

Then,= −6 × 96487 C mol−1 × 0.34 V

= −196833.48 CV mol−1

= −196833.48 J mol−1

= −196.83 kJ mol−1

Again,

= −RT ln K

=34.496

K = antilog (34.496)

=3.13 × 1034

(ii)

Thegalvanic cell of the given reaction is depicted as:

Now,the standard cell potential is

Here,n = 1.

Then,

= −1 × 96487 C mol−1 × 0.03 V

= −2894.61 J mol−1

= −2.89 kJ mol−1

Again,

=0.5073

K= antilog (0.5073)

= 3.2 (approximately)

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