The cell reaction is |
\[Z{{n}_{(s)}}+Cu_{(aq)}^{2+}\xrightarrow[{}]{{}}Zn_{(aq)}^{2+}+C{{u}_{(s)}}\] |
A) \[-412.8\]
B) 192.0
C) \[-384.0\]
D) 206.4
Correct Answer: A
Solution :
\[{{\Delta }_{r}}{{H}^{o}}=-nF{{E}^{o}}+nFT\left( \frac{\Delta {{E}^{o}}}{\Delta T} \right)\] \[=-2\times 96000\times 2+2\times 96000\times 300(-5\times {{10}^{-4}})\] \[=-384000-28800=-412.8kJ\,mo{{l}^{-1}}\]You need to login to perform this action.
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