Question

For the reaction below:

PCl₅​(g)⇌PCl₃​(g)+Cl₂​(g)
The equilibrium constant K is found to be 1.0×10⁻³. What is ΔG⁺ (in kilojoules per mole) for this reaction at 298 K ?
Remember to use correct significant figures in your answer (round your answer to the nearest whole number). Do not include units in your response.
Provide your answer below:

Answer 1

The ΔG⁺ for the reaction PCl₅​(g)⇌PCl₃​(g)+Cl₂​(g) at 298 K is -56 kJ/mol.

Step-by-step explanation:

The equilibrium constant (K) for the reaction is 1.0×10⁻³ at 298 K. To calculate the standard free energy change (ΔG⁺) for the reaction, you can use the formula: ΔG⁺ = -RT ln(K), where R is the gas constant (8.314 J/mol K) and T is the temperature in Kelvin (298 K).

Plugging in the values, we get: ΔG⁺ = -8.314 J/mol K × 298 K × ln(1.0×10⁻³) = -55.7 kJ/mol. Since the question asks for the answer in kilojoules per mole, we can round the answer to -56 kJ/mol.