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Chemistry - Thermodynamics - II Question with Solution | TestHub

ChemistryThermodynamics - IIFree Energy and EquilibriumMedium2 minQB

ChemistryMediumsingle choice

The standard Gibbs energy change at 300 K for the reaction $2 X ⇌ Y + Z$ is $- 2494.2 J$ . At a given time the composition of the mixture is $[X] = 2$ , $[Y] = 2$ and $[Z] = 1$ . The reaction proceeds in the: [ $R = 8.314 J/K/mol$ , $e = 2.718$ ]

Options:

Answer:

Solution:

$ln K_{c} = - \frac{Δ G ^{\circ}}{RT} = \frac{2494.2}{8.314 \times 300} = 1$ , so $K_{c} = e = 2.718$ .

$Q = \frac{[ Y ] [ Z ]}{[ X ] ^{2}} = \frac{2 \times 1}{4} = 0.5$ .

$Q < K_{c}$ , so the reaction proceeds in the forward direction.

Answer: (A).

Stream:JEESubject:ChemistryTopic:Thermodynamics - IISubtopic:Free Energy and Equilibrium

⏱ 2mℹ️ Source: QB

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