For the reaction,
2 A(g)+ B(g) $\to$ 2D(g), $△ U^{⊖} = - 10.5 K J$ and $△ S^{⊖} = - 44.1 J K^{- 1}$

Calculate $△ G^{⊖}$ for the reaction and predict whether the reaction may occur spontaneously.

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Solution

The change in the number of moles of gaseous species, $Δ n_{g} = 2 - 3 = - 1$

$Δ H^{0} = Δ U^{0} + Δ n_{g} R T = - 10.5 + (- 1) \times 8.314 \times 10^{- 3} \times 298 = - 12.98 k J$
$Δ G^{0} = Δ H^{0} - T Δ S^{0} = - 12.98 - 298 (- 44.10 \times 10^{- 3}) = 0.16 k J$

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Similar questions

Q. For the reaction,

2 A (g) + B (g) ⟶ 2 D (g), Δ U = - 10.5 K J

and

Δ S = - 44.10 J K^{- 1}

. Calculate

Δ G

for the reaction and reaction and predict whether the reaction may occur spontaneously.

For the reaction

2A₍_g₎ + B₍_g₎ → 2D₍_g₎

ΔU^θ = –10.5 kJ and ΔS^θ= –44.1 JK^–1.

Calculate ΔG^θ for the reaction, and predict whether the reaction may occur spontaneously.

Q. a) For the reaction :

2 A (g) + B (g) ⟶ 2 D (g)

Δ U = - 10.5 k J

and

Δ S = - 44.1 {k J}^{- 1}

. Calculate

Δ G

for the reaction, and predict whether the reaction may occur spontaneously.
b) Predict whether the reaction is spontaneous or not at high temperature.

For the reaction
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Calculate $Δ G^{θ}$ for the reaction, and predict whether the reaction may occur spontaneously.

Q. For the reaction:

2 A (g) + B (g) \to 2 D (g)

Δ U^{⊖} = - 10.5

kJ and

Δ S^{⊖} = - 44.1

J K^{- 1}

.Does the reaction occur spontaneously?

[Give your answer in terms of Yes or No]

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For the reaction,2 A(g)+ B(g) → 2D(g), △U⊖=−10.5KJ and △S⊖=−44.1JK−1Calculate △G⊖ for the reaction and predict whether the reaction may occur spontaneously.

The change in the number of moles of gaseous species, Δng=2−3=−1ΔH0=ΔU0+ΔngRT=−10.5+(−1)×8.314×10−3×298=−12.98kJΔG0=ΔH0−TΔS0=−12.98−298(−44.10×10−3)=0.16kJ

For the reaction,
2 A(g)+ B(g) $\to$ 2D(g), $△ U^{⊖} = - 10.5 K J$ and $△ S^{⊖} = - 44.1 J K^{- 1}$

Calculate $△ G^{⊖}$ for the reaction and predict whether the reaction may occur spontaneously.

The change in the number of moles of gaseous species, $Δ n_{g} = 2 - 3 = - 1$

$Δ H^{0} = Δ U^{0} + Δ n_{g} R T = - 10.5 + (- 1) \times 8.314 \times 10^{- 3} \times 298 = - 12.98 k J$
$Δ G^{0} = Δ H^{0} - T Δ S^{0} = - 12.98 - 298 (- 44.10 \times 10^{- 3}) = 0.16 k J$