Question

For the cell reaction: $2C{u^{+}}_{(aq)} \rightarrow Cu_{(s)} + Cu_{(aq)}^{2 +}$ the standard cell potential is $0.36V$ the equilibrium constant for the reaction is

• A. $1.2 \times 10^{6}$
• B. $7.4 \times 10^{12}$
• C. $2.4 \times 10^{6}$
• D. $5.5 \times 10^{8}$

Answer 1

Answer: (A)

$1.2 \times 10^{6}$

Answer 2

$\log K_{c} = \frac{nEº_{cell}}{0.0591}$

For the given reaction n = 1

$\log K_{c} = \frac{1 \times 0.36}{0.0591} = 6.09$

$K_{c} = anti\log 6.09 = 1.2 \times 10^{6}$