| For the cell reaction [NEET 2019] |
| \[2F{{e}^{3+}}(aq)+2{{I}^{}}(aq)\to 2F{{e}^{2+}}(aq)+{{I}_{2}}(aq)\]\[E_{cell}^{\Theta }\text{ }E=0.24\text{ }Vat\text{ }298\text{ }K\]. The standard Gibbs energy \[({{\Delta }_{r}}{{G}^{\Theta }})\] of the cell reaction is: |
| [Given that Faraday constant\[F=96500\text{ }C\text{ }mo{{l}^{1}}\]] |
A) \[46.32\text{ }kJ\text{ }mo{{l}^{1}}\]
B) \[23.16\text{ }kJ\text{ }mo{{l}^{1}}\]
C) \[-46.32\text{ }kJ\text{ }mo{{l}^{1}}\]
D) \[-23.16\text{ }kJ\text{ }mo{{l}^{1}}\]
Correct Answer: C
Solution :
| [c] \[\Delta G{}^\circ =-nF\,E_{cell}^{\Theta }\] |
| \[=2(96500)\,\text{(}0.24\text{)}\] |
| \[=-46320\text{ }J/mole\] |
| \[=-\frac{46320}{1000}\] |
| \[=-46.32\text{ }KJ/mole\] |
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