Question

The equilibrium constant of the reaction:

Cu(s) + 2Ag⁺(aq) -) Cu²⁺(aq) + 2Ag(s);

E° = 0.46 V at 298 K is

(a) 2.0 x 10¹⁰

(b) 4.0 x 10¹⁰

(c) 4.0 x 10¹⁵

(d) 2.4 x 10¹⁰

Answer 1

Correct option (c) 4.0 x 10¹⁵

Explanation :

For a cell reaction in equilibrium at 298 K,

where KC = equilibrium constant, n = number of electrons involved in the electrochemical cell reaction.

Answer 2

Correct option is (c) 4.0 x 10¹⁵

Cu(s) + 2Ag²⁺(aq) ⟶ Cu²⁺(aq) + 2Ag(s)

E^o = 0.46V at 298K

log K_C​ = \(\frac{nFE^o}{RT}\)

\(= \frac{2\times 0.46}{0.059}\)

K_C​ = 4 × 10¹⁵