For the reaction- 2Ag-Bg- 2Dg- - U-10-5 kJ and - S-44-1 JK-1-Does the reaction occur spontaneously-Give your answer in terms of Yes or No-

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Standard XII

Chemistry

Spontaneity

For the react...

Question

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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Solution

Given:-
$Δ U^{0} = - 10.5 k J$
$Δ S^{0} = - 44.1 J / K$
$2 A_{(g)} + B_{(g)} ⟶ 2 D_{(g)}$

For the above reaction-
$Δ n_{g} = 2 - (2 + 1) = - 1$

As we know that,
$Δ H^{0} = Δ U^{0} + Δ n_{g} R T$
$Δ H^{0} = - 10.5 + (- 1 \times 8.314 \times 10^{- 3}) (298)$
$\Rightarrow Δ H^{0} = - 12.98 k J$

Again as we know that,
$Δ G^{0} = Δ H^{0} - T Δ S^{0}$
$\Rightarrow Δ G^{0} = - 12.98 - 298 \times (- 44.1 \times 10^{- 3}) = + 0.16 k J$

Since $Δ G^{0}$ for the reaction is positive, the reaction will not occur spontaneously.

Hence the correct answer is No.

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For the reaction:2A(g)+B(g)→2D(g), ΔU⊖=−10.5 kJ and ΔS⊖=−44.1 JK−1.Does the reaction occur spontaneously?[Give your answer in terms of Yes or No]

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]