The standard reaction Gibbs energy for a chemical reaction at an absolute temperature T is given by Δ G ∘ = A − BT where A and B are non-zero constants. Which of the following is true about this reaction?

Δ G ∘ = A − BT A and B are non-zero constants ∴ Δ G ∘ = Δ H ∘ − T Δ S ∘ = A − BT ∴ Reaction will be endothermic if Δ G ∘ > 0. Hence, A > 0 and B < 0

Chemistry - Thermodynamics - II Question with Solution | TestHub

ChemistryThermodynamics - IIFree Energy and EquilibriumHard2 minPYQ_2019

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The standard reaction Gibbs energy for a chemical reaction at an absolute temperature $T$ is given by $Δ G^{\circ} = A - BT$ where A and $B$ are non-zero constants. Which of the following is true about this reaction?

Options:

Answer:

Solution:

$Δ G^{\circ} = A - BT$ A and B are non-zero constants $∴ Δ G^{\circ} = Δ H^{\circ} - T Δ S^{\circ} = A - BT$ $∴$ Reaction will be endothermic if $Δ G^{\circ} > 0.$ Hence, $A > 0$ and $B < 0$

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

⏱ 2mℹ️ Source: PYQ_2019

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