Question

Assume a cell with the following reaction

$C{u}_{\left(s\right)}+2A{g}^{+}(1\times {10}^{-3}M)\to C{u}^{2+}\left(0.250M\right)+2Ag\left(s\right)$

$E_{cell}^0=2.97V$

$E_{cell}$ for the above reaction is ____V. (Nearest integer)
[Given : $log2.=0.3979,T=298K$]

• A. 3.0
• B. 3.00
• C. 3

Answer 1

Answer: (A), (B), (C)

$Cu+2A{g}^{+}⟶C{u}^{2+}+2Ag$

${10}^{-3}M0.25M$

$E_{cell}=E_{cell}^0-\frac{0.059}{2}log\frac{\left[C{u}^{2+}\right]}{[A{g}^{+}{]}^2}$

$E_{cell}=2.97-\frac{0.059}{2}log\frac{\left(0.25\right)}{({10}^{-3}{)}^2}$

$E_{cell}=2.97-0.16E_{cell}=2.81V$
Nearest integer is 3