For the reaction I₂(s) + Cl₂(g) → 2 ICl(g) ΔH = 36 kJ and ΔS = 158.8 J/K at 25°C. Calculate the temperature at which Keq is 4.0 × 10³. A) 128 °C B) -115 °C C) 83 °C D) 25 °C E) -175 °C

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The correct answer is A.The equilibrium constant Keq is given by the expression:Keq = [ICl]^2 / [I2][Cl2]The change in free energy ΔG is given by the expression:ΔG = -RTlnKeqwhere R is the gas constant (8.314 J/mol·K) and T is the temperature in Kelvin.The change in enthalpy ΔH and the change in entropy ΔS are related to ΔG by the expression:ΔG = ΔH - TΔSAt equilibrium, ΔG = 0, so we can solve for the temperature T:T = ΔH / ΔSSubstituting the given values, we get:T = 36 kJ / 158.8 J/K = 226.7 K = -46.3 °CConverting to Celsius, we get:T = -46.3 °C + 273.15 = 226.85 °CTherefore, the temperature at which Keq is 4.0 × 10^3 is 226.85 °C, which is closest to choice A, 128 °C.

For the Reaction I2(s) + Cl2(g) → 2 ICl(g)

For the Reaction I₂(s) + Cl₂(g) → 2 ICl(g)