QNEET-2024-Ch-109: NEET 2024 Chemistry - Class 12 NEET-2024-Ch-109 Solution: The standard cell potential of the following cell \(Zn

To find the standard Gibbs energy change for the reaction, we can use the relationship between the standard Gibbs free energy change ( _ G _ ) and the standard cell potential ( E _ ) given by the following equation: _ G _ = _ n F E _ Where: n is the number of moles of electrons transferred in the reaction. F is the Faraday constant ( 1   F = 96487   C _ mol _ 1 ). E _ is the standard cell potential. From the given reaction: Zn ( s ) + Fe 2 + ( aq ) _ Zn 2 + ( aq ) + Fe ( s ) It can be observed that n = 2 because two electrons are transferred from zinc to iron. Given data: E _ = 0.32   V 1   F = 96487 C / mol Now, substitute the values into the equation: _ G _ = _ n F E _ _ G _ = _ 2 _ 96487   C / mol _ 0.32   V Calculate the value: _ G _ = _ 2 _ 96487   C / mol _ 0.32   V _ G _ = _ 2 _ 30875.84   J / mol _ G _ = _ 61751.68   J / mol Converting the units to kJ/mol: _ G _ = _ 61.75168   kJ / mol The closest answer, when rounded to two decimal places, is: _ G _ = _ 61.75   kJ / mol Therefore, the correct option is: Option A: _ 61.75   kJ   mol _ 1