STANDARD Chemistry Gibbs Free Energy MCQ Question
The equilibrium constant for a reaction is 10. What will be the value of ΔG° at 300 K?
-5.74 kJ
-574 kJ
+11.48 kJ
+5.74 kJ
Correct Answer
Detailed Explanation
The Gibbs free energy change is calculated using the formula ΔG° = -RT ln K. Substituting the given values, ΔG° = -2.303 × 8.314 × 300 × log 10 = -5744.1 J = -5.74 kJ.
Found an issue with this question?
Related Questions
More from Chemical Equilibrium
For the forward chemical reaction, A + B ⇌ C, The rate of reaction is, Kₑ = [C]/[A][B] And for reverse chemical reaction, C ⇌ A + B, The rate of react...
The equilibrium constants of the following are: N₂ + 3H₂ ⇌ 2NH₃ ; K₁ N₂ + O₂ ⇌ 2NO ; K₂ H₂ + 1/2 Ω₂ ⇌ H₂O ; K₃ The equilibrium constant (K) of the rea...
We know that the relationship between Kc and Kp is : Kp = Kc(RT)Δn What would be the value of Δn for the reaction: NH₄Cl(s) ⇌ NH₃(g) + HCl(g) ?