
- A

- ✓

- C

- D







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$Time (sec)$ Rate $(mol\, L^{-1} sec.^{-1})$
$0$ $1.60 \times 10^{-2}$
$10$ $1.60 \times 10^{-2}$
$20$ $1.60 \times 10^{-2}$
$30$ $1.60 \times 10^{-2}$
From the above data, the order of reaction is
$\mathrm{Cu}_{(\mathrm{s})}+2 \mathrm{Ag}^{+}\left(1 \times 10^{-3} \,\mathrm{M}\right) \rightarrow \mathrm{Cu}^{2+}(0.250\, \mathrm{M})+2 \mathrm{Ag}_{(\mathrm{s})}$
$\mathrm{E}_{\mathrm{Cell}}^{\ominus}=2.97\, \mathrm{~V}$
$\mathrm{E}_{\text {cell }}$ for the above reaction is $....\,V.$ (Nearest integer)
[Given : $\log 2.5=0.3979, T=298\, \mathrm{~K}]$
