A) \[-108.08\,kJ\]
B) \[108.08\,kJ\]
C) \[121.31\,kJ\]
D) \[-121.31\,kJ\]
Correct Answer: A
Solution :
[a]\[Pb|PbC{{l}_{2}}||AgCl||Ag\] |
The cell reaction is |
\[Pb+2AgCl\xrightarrow{{}}PbC{{l}_{2}}+2Ag\] |
\[\Delta G=-nFE\] |
\[=-\,2\times 96500\times 0.5J\] |
\[=-\,96500J\]or \[-\,96.5kJ\] |
\[\Delta S=nF{{\left( \frac{\partial E}{\partial T} \right)}_{p}}\] |
\[=2\times 96500\times -2\times {{10}^{-\,4}}\] |
\[=-\,38.6J{{K}^{-1}}\] |
Also, \[\Delta G=\Delta H-T\Delta S\] |
\[=-\,96500\] |
\[=\Delta H-300\,(-38.6)\] |
\[=\Delta H=-\,96500-300\times 38.6\] |
\[=-108080J\] |
\[=-108.08\,kJ\] |
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