Question

Calculate the equilibrium constant at 25 °C for each of the following reactions from the value of ΔG° given.

(a) I₂(s) + Cl₂(g) ⟶ 2ICl(g) ΔG° = −10.88 kJ

(b) H₂(g) + I₂(s) ⟶ 2HI(g) ΔG°=3.4 kJ

(c) CS₂(g) + 3Cl₂(g) ⟶ CCl₄(g) + S₂Cl₂(g) ΔG°=−39 kJ

(d) 2SO₂(g) + O₂(g) ⟶ 2SO₃(g) ΔG°=−141.82 kJ

(e) CS₂(g) ⟶ CS₂(l) ΔG°=−1.88 kJ

Answer 1

The equilibrium constants for the given reactions can be calculated using the equation Kc = e^(-ΔG°/RT). The equilibrium constants at 25°C for the reactions (a) to (e) are 7.59 × 10⁶, 1.25 × 10², 2.34 × 10⁻⁴, 2.60 × 10⁻¹⁹, and 1.25 × 10⁷, respectively.

Step-by-step explanation:

The equilibrium constant, Kc, can be calculated from the value of ΔGo using the equation: Kc = e-ΔGo/RT.

Using this equation, we can calculate the equilibrium constants for the given reactions:

1. (a) Kc = e-(-10.88 kJ / (8.314 J/mol·K * (25 + 273) K)) = 7.59 × 10⁶
2. (b) Kc = e-((3.4 kJ) / (8.314 J/mol·K * (25 + 273) K)) = 1.25 × 10²
3. (c) Kc = e-(-39 kJ / (8.314 J/mol·K * (25 + 273) K)) = 2.34 × 10⁻⁴
4. (d) Kc = e-(-141.82 kJ / (8.314 J/mol·K * (25 + 273) K)) = 2.60 × 10⁻¹⁹
5. (e) Kc = e-(-1.88 kJ / (8.314 J/mol·K * (25 + 273) K)) = 1.25 × 10⁷