For the reaction given below the values of standard Gibbs free energy of formation at 298 K are given. What is the nature of the reaction? I2 + H2S → 2HI + S Δ G°f(HI) = 1.8 kJ mol-1, Δ G° f(H2S) = 33.8 kJ mol-1

Question

For the reaction given below the values of standard Gibbs free energy of formation at 298 K are given. What is the nature of the reaction? I2 + H2S → 2HI + S Δ G°f(HI) = 1.8 kJ mol-1, Δ G° f(H2S) = 33.8 kJ mol-1 (A) Non-spontaneous in forward direction (B) Spontaneous in forward direction (C) Spontaneous in backward direction (D) Non-spontaneous in both forward and backward directions

Tardigrade Admin · Accepted Answer

I2 + H2S → 2HI + S Δ G° = Sigma G°f(Products) - Sigma G°f(Reactants) Δ G° = (2 × 1.8 + 0) - (0 + 33.8) = -30.2 kJ Hence, reaction is spontaneous in forward direction.

Q. For the reaction given below the values of standard Gibbs free energy of formation at $298 K$ are given. What is the nature of the reaction?
$I_{2} + H_{2} S \to 2 H I + S$
$Δ G_{f}^{\circ} (H I) = 1.8 k J m o l^{- 1}$ , $Δ G_{f}^{\circ} (H_{2} S) = 33.8 k J m o l^{- 1}$

Non-spontaneous in forward direction

Spontaneous in forward direction

Spontaneous in backward direction

Non-spontaneous in both forward and backward directions

$I_{2} + H_{2} S \to 2 H I + S$
$Δ G^{\circ} = Σ G_{f (P ro d u c t s)}^{\circ} - Σ G_{f (R e a c t an t s)}^{\circ}$
$Δ G^{\circ} = (2 \times 1.8 + 0) - (0 + 33.8) = - 30.2 k J$
Hence, reaction is spontaneous in forward direction.

Q. For the reaction given below the values of standard Gibbs free energy of formation at 298K are given. What is the nature of the reaction? I2​+H2​S→2HI+S ΔGf∘​(HI)=1.8kJmol−1, ΔGf∘​(H2​S)=33.8kJmol−1