A) \[-\,0.3125\,\text{V}\]
B) \[0.3125\,\text{V}\]
C) \[1.114\,\text{V}\]
D) \[-\,1.114\text{V}\]
Correct Answer: B
Solution :
Species with more negative \[{{\text{E}}^{\text{o}}}\](standard reduction potential) generally acts as reducing agent while with less negative \[{{\text{E}}^{\text{o}}}\]acts as oxidising agent. Thus, the overall reaction is \[\text{A}{{\text{g}}^{+}}+F{{e}^{2+}}\xrightarrow{{}}F{{e}^{3+}}+Ag\] \[\Delta {{E}^{o}}={{E}^{o}}_{OA}-{{E}^{o}}_{RA}\] \[=-0.3995-(-0.7120)\,V\] \[=-0.3995+\,0.7120\,V\] \[=+\,0.3125\,V\]You need to login to perform this action.
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