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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