The equilibrium constant for the formation of hydrogen iodide from hydrogen and iodine is 45.0 at a certain temperature. H₂(g) + I₂(s) 2 HI(g)
Which of the following is true regarding this equilibrium?
I.The reaction is product-favored.
II.The reaction is reactant-favored.
III.Equilibrium lies to the right.
IV.Equilibrium lies to the left.

Question

The equilibrium constant for the formation of hydrogen iodide from hydrogen and iodine is 45.0 at a certain temperature. H₂(g) + I₂(s)

The equilibrium constant for the formation of hydrogen iodide from hydrogen and iodine is 45.0 at a certain temperature. H<sub>2</sub>(g) + I<sub>2</sub>(s) 2 HI(g) Which of the following is true regarding this equilibrium? I.The reaction is product-favored. II.The reaction is reactant-favored. III.Equilibrium lies to the right. IV.Equilibrium lies to the left. A) I and III B) I and IV C) II and III D) II and IV E) None are true, as the concentrations of reactants and products are essentially the same.

2 HI(g)
Which of the following is true regarding this equilibrium?
I.The reaction is product-favored.
II.The reaction is reactant-favored.
III.Equilibrium lies to the right.
IV.Equilibrium lies to the left.

Quizplus · Accepted Answer

The equilibrium constant, K = [HI]2/([H2]*[I2]), is 45.0, which means at equilibrium, [HI] is larger compared to [H2] and [I2]. This also means that the numerator is much larger than the denominator, indicating that the reaction is product-favored. Therefore, choices (I) and (III) are correct. Choices (II) and (IV) are incorrect. Hence, the answer is (A).

The Equilibrium Constant for the Formation of Hydrogen Iodide from Hydrogen