For a certain reaction at 300 K, K=10, then ΔG∘ for the same reaction is _______ ×10−1 kJ mol−1
Question
Solution
To find the ΔG∘ for the reaction, we can use the formula:
ΔG∘ = -RT ln K
Where: R is the gas constant, which is 8.314 J/(mol·K) or 0.008314 kJ/(mol·K) T is the temperature in Kelvin, which is 300 K K is the equilibrium constant, which is 10
Substituting the values into the formula, we get:
ΔG∘ = - (0.008314 kJ/(mol·K) * 300 K * ln 10)
Solving this, we get:
ΔG∘ = -5.708 kJ/mol
However, the question asks for the answer in terms of ×10−1 kJ mol−1. To convert, we simply multiply the answer by 10:
ΔG∘ = -5.708 * 10 = -57.08 ×10−1 kJ mol−1
So, the ΔG∘ for the reaction is -57.08 ×10−1 kJ mol−1.
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