For a gaseous reaction A + 3 B ⇌ 2 C ; Δ H ∘ = − 90 K J Δ S ∘ = − 200 JK − 1 at 400 K . For the reaction 2 1 A + 2 3 B ⇌ C at 400 K , magnitude of Δ G ∘ (in kJ ) is:

A + 3 B ⇌ 2 C Δ G ∘ = Δ H ∘ − T Δ S ∘ = − 90 − 400 × ( − 0.200 ) = − 90 + 80 = − 10 k J . \displaylines ∴ F or 2 1 A + 2 3 B ⇌ C Δ G ∘ = − 5 K J

Chemistry - Thermodynamics - II Question with Solution | TestHub

ChemistryThermodynamics - IIGibb's Free EnergyMedium2 min

ChemistryMediuminteger

For a gaseous reaction

$A + 3 B ⇌ 2 C; Δ H^{\circ} = - 90 K J$

$Δ S^{\circ} = - 200 JK^{- 1}$ at 400 K .

For the reaction $\frac{1}{2} A + \frac{3}{2} B ⇌ C$ at 400 K ,

magnitude of $Δ G^{\circ}$ (in kJ ) is:

Answer:

Solution:

$A + 3 B ⇌ 2 C$

$Δ G^{\circ} = Δ H^{\circ} - T Δ S^{\circ}$

$= - 90 - 400 \times (- 0.200)$

$= - 90 + 80 = - 10 k J .$

$\displaylines ∴ F or \frac{1}{2} A + \frac{3}{2} B ⇌ C Δ G^{\circ} = - 5 K J$

Stream:JEESubject:ChemistryTopic:Thermodynamics - IISubtopic:Gibb's Free Energy

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