Which of the following reactions will be spontaneous in an electrochemical cell constructed from the given standard electrode potentials: $E_{Cl_2 \mid 2Cl^-}^0 = 1.36 \ V$ and $E_{Br_2 \mid 2Br^-}^0 = 1.09 \ V$?
- A$2Cl^- + 2Br^- \rightarrow Cl_2 + Br_2$
- B$2Br^- + Cl_2 \rightarrow Br_2 + 2Cl^-$
- C$Br_2 + 2Cl^- \rightarrow 2Br^- + Cl_2$
- D$Cl_2 + Br_2 \rightarrow 2Cl^- + 2Br^-$
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Standard electrode potential of $Ag^{+}/Ag$ and $Cu^{2+}/Cu$ is $+0.80 \ V$ and $+0.34 \ V$ respectively. These electrodes are joined together by a salt bridge. If:
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View SolutionCalculate the standard cell potential (in $V$) of the cell in which the following reaction takes place:
$Fe^{2+}_{(aq)} + Ag^{+}_{(aq)} \to Fe^{3+}_{(aq)} + Ag_{(s)}$
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$E^o_{Ag^{+}/Ag} = x \ V$
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