For the cell reaction: 2Cu+(aq) → Cu(s)+Cu2+(aq), the standard cell potential is 0.36 V. The equilibrium constant for the reaction is

Question

For the cell reaction: 2Cu+(aq) → Cu(s)+Cu2+(aq), the standard cell potential is 0.36 V. The equilibrium constant for the reaction is (A) 1.2×106 (B) 7.4×1012 (C) 2.4×106 (D) 5.5×108

Tardigrade Admin · Accepted Answer

log Kc=(nE°cell/0.0591) For the given reaction, n = 1 log Kc=(1×0.36/0.0591)=6.09 Kc= antilog 6.09=1.2×106

Q. For the cell reaction : $2 C u_{(a q)}^{+} \to C u_{(s)} + C u_{(a q)}^{2 +}$ , the standard cell potential is $0.36 V$ . The equilibrium constant for the reaction is

$1.2 \times 1 0^{6}$

$7.4 \times 1 0^{12}$

$2.4 \times 1 0^{6}$

$5.5 \times 1 0^{8}$

$l o g K_{c} = \frac{n E _{ce ll}^{\circ}}{0.0591}$
For the given reaction, $n = 1$
$l o g K_{c} = \frac{1 \times 0.36}{0.0591} = 6.09$
$K_{c} =$ antilog $6.09 = 1.2 \times 1 0^{6}$

Q. For the cell reaction : 2Cu(aq)+​→Cu(s)​+Cu(aq)2+​, the standard cell potential is 0.36V. The equilibrium constant for the reaction is

1.2×106

7.4×1012

2.4×106

5.5×108