For the reaction- 2Ag-Bg- 2Dg- U -10-5KJ and - S -44-10J K -1- Calculate - G for the reaction and reaction and predict whether the reaction may occur spontaneously-

Let T=298 Δ H=Δ U+AngRT = 10500 1× 8.314× 298 = 10500 2477.572 Δ H= 12977.572 Δ G=Δ H TΔ S = 12977.572( 298× 44.1) = 129 ...

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Spontaneity

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Question

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.

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2 A (g) + B (g) ⟶ 2 D (g)

Δ U = - 10.5 k J

Δ S = - 44.1 {k J}^{- 1}

Δ G

\to

△ U^{⊖} = - 10.5 K J

△ S^{⊖} = - 44.1 J K^{- 1}

△ G^{⊖}

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.

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

Δ U^{⊖} = - 10.5

Δ S^{⊖} = - 44.1

J K^{- 1}

Δ U

2 A (g) + B (g) ⇌ A_{2} B (g)

K_{p} = 1.0 \times 10^{- 10} {a t m}^{- 2}

Δ S = 5 J K^{- 1}

T = 300 K

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