For the reaction 2HF(g) H₂(g) + F₂(g), ΔG° = 38.3 kJ at 1000 K. If, at this temperature, 5.00 mol of HF(g), 0.500 mol of H₂(g), and 0.75 mol of F₂(g) are mixed in a 1.00-L container:

Question

Quizplus · Accepted Answer

The given value of ΔG° indicates that the reaction is thermodynamically favorable in the forward direction. However, the question asks about the direction of the reaction in a specific mixture of reactants. To determine the direction of the reaction, we can calculate the reaction quotient Q and compare it to the equilibrium constant K. At 1000 K, the expression for Q is: Q = [H₂]^2 [F₂] / [HF]^2 = (0.5)^2 (0.75) / (5.00)^2 = 0.00375 We can calculate the equilibrium constant K using the following equation: ΔG° = -RT ln K where R is the gas constant (8.314 J/mol-K) and T is the temperature in Kelvin. ΔG° = 38.3 kJ = - (8.314 J/mol-K) (1000 K) ln K Solving for K, we find: K = 1.10 x 10^15 Since Q < K, the reaction proceeds in the forward direction to reach equilibrium. This means that some HF will be formed from H₂ and F₂ until Q reaches the value of K. Therefore, the best choice is A.

For the Reaction 2HF(g) H2(g) + F2(g), ΔG° =

For the Reaction 2HF(g) H₂(g) + F₂(g), ΔG° =