For the reaction 2H2S(g) + 3O2(g) → 2H2O(l) + 2SO2(g) ΔH∘ = −1124.0 kJ

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For the reaction 2H2S(g) + 3O2(g) → 2H2O(l) + 2SO2(g) ΔH∘ = −1124.0 kJ and ΔS∘ = −390.7 J/K The standard free energy change for the reaction of 2.47 moles of H2 S(g) at 347 K, 1 atm would be kJ. This reaction is favored under standard conditions at 347 K. Assume that ΔH∘ and ΔS∘ are independent of temperature.

For the reaction 2H2S(g) + 3O2(g) → 2H2O(l) + 2SO2(g) ΔH∘ = −1124.0 kJ and ΔS∘ = −390.7 J/K The standard free energy change for the reaction of 2.47 moles of H2 S(g) at 347 K, 1 atm would be kJ. This reaction is favored under standard conditions at 347 K. Assume that ΔH∘ and ΔS∘ are independent of temperature.

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For the reaction

\begin{matrix} 2 H_{2} S (g) + 3 O_{2} (g) \to 2 H_{2} O (l) + 2 {S O}_{2} (g) \\ Δ H^{\circ} = - 1124.0 k J and Δ S^{\circ} = - 390.7 J / K \end{matrix}

The standard free energy change for the reaction of 2.47 moles of

H_{2} S (g)

at

347 K, 1

atm would be

◻

kJ.

This reaction is

◻

favored under standard conditions at

347 K

. Assume that

Δ H^{\circ}

and

Δ S^{\circ}

are independent of temperature.

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