$Ag\left( s \right)/A{g^ \oplus }||C{u^{2 + }}/Cu\left( s \right)$
$A{g^ \oplus } + {e^ - } \to Ag\,;\,{E^o} = x$
$C{u^{2 + }} + 2{e^ - } \to Cu\,;\,{E^o} = y$
$E^o_{cell}$ is
$E_{\text {Cell }}^{0}=\mathrm{y}-\mathrm{x}$
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In the above first order reaction the initial concentration of $\mathrm{N}_{2} \mathrm{O}_{5}$ is $2.40 \times 10^{-2}\, \mathrm{~mol} \,\mathrm{~L}^{-1}$ at $318 \,K.$ The concentration of $\mathrm{N}_{2} \mathrm{O}_{5}$ after $1\, hour$ was $1.60 \times 10^{-2}\, \mathrm{~mol} \,\mathrm{~L}^{-1}$, The rate constant of the reaction at $318\, \mathrm{~K}$ is $.....\,\times 10^{-3} \mathrm{~min}^{-1}$. (Nearest integer)
[Given: $\log 3=0.477, \log 5=0.699$ ]
Product $(b)$ of above reaction is
