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Question

In a fuel cell (the device used for producing electricity directly from a chemical reaction) methanol is used as a fuel and oxygen gas is used as an oxidizer. The standard enthalpy of combustion of methanol is 726kJmol1. The standard free energies of formation of CH3OH(l).CO2(g) and H2O(l) are 166.3,394.4 and 237.1kJmol1 respectively.
The standard free energy change of the reaction will be:

A
597.8kJmol1
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B
298.9kJmol1
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C
465.2kJmol1
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D
702.3kJmol1
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Solution

The correct option is C 465.2kJmol1
Solution:- (C) 465.2kJ/mol
CH3OH(l)+32O2(g)CO2(g)+2H2O(l)
Given:-
ΔG0f(CH3OH(l))=166.3kJ/mol
ΔG0f(CO2(l))=394.4kJ/mol
ΔG0f(H2O(l))=237.1kJ/mol
Therefore,
ΔG0Reaction=ΔG0f(product)ΔG0f(reactant)
ΔG0Reaction=(ΔG0f(CO2(l))+ΔG0f(H2O(l)))ΔG0f(CH3OH(l))
ΔG0Reaction=((394.4)+(237.1))(166.3)
ΔG0Reaction=465.2kJ/mol
Hence the standard free energy change of the reaction will be 465.2kJ/mol.

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