| For the reduction of silver ions with copper metal, the standard cell potential was found to be \[+\text{ }0.46\,V\] at \[25{}^\circ C\] |
| The value of standard Gibbs energy, \[\Delta {{G}^{o}}\] will be \[(F\text{ }=\text{ }96500\text{ }C\text{ }mo{{l}^{-1}})\] [AIPMT (S) 2010] |
A) \[-89.0\text{ }kJ\]
B) \[-89.0\text{ }J\]
C) \[-44.5\text{ }kJ\]
D) \[-98.0k\text{ }J\]
Correct Answer: A
Solution :
| [a] We know that, standard Gibbs energy,\[\Delta {{G}^{o}}=-nF{{E}^{o}}_{cell}\] For the cell reaction, |
| \[2A{{g}^{+}}+Cu\xrightarrow[{}]{{}}C{{u}^{2+}}+2Ag\] |
| \[\Delta E_{cell}^{o}=+\,0.46\,\text{V}\] |
| \[\Delta {{G}^{o}}=-2\times 96500\times 0.46\] |
| \[=-88780\,\text{J}\] |
| \[=-88.7\,\text{kJ}\,\text{K}\approx -\text{89}\text{.0}\,\text{kJ}\] |
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