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  • Given the equilibrium constant: KC of the reaction:- <img alt="\mathrm{Cu}(\mathrm{s})+2 \mathrm{Ag}^{+}(\mathrm{aq}) \rightarrow \mathrm{Cu}^{2+}(\mathrm{aq})+2 \mathrm{Ag}(\mathrm{

Given the equilibrium constant: KC of the reaction:-

\mathrm{Cu}(\mathrm{s})+2 \mathrm{Ag}^{+}(\mathrm{aq}) \rightarrow \mathrm{Cu}^{2+}(\mathrm{aq})+2 \mathrm{Ag}(\mathrm{s})  is  \mathrm{ 10 \times 10^7} . Calculate the \mathrm{ E^0}cell of this rxn at   \mathrm{ 298 k\left\{2.303 \frac{R T}{F}\right.at \left.298 K=0.059 \mathrm{~V}\right\}}.

Option: 1

 0.414 


Option: 2

 0.362 


Option: 3

0.236 
 


Option: 4

0.41


Answers (1)

best_answer

\mathrm{E_{\text {cell }}^0=\frac{2.303RT}{nF } \log k c}

\mathrm{E_{\text {cell }}^0=\frac{0.59 V}{n } \log k c}

\mathrm{ E^{0}_{\text {cell }}=\frac{0.059 \mathrm{V}}{2} \log 10 ^{8}}
\mathrm{ E^{0}_{\text {cell }}=0 .236 }.

 

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