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 (Kc) value of 45.0 indicates a strong preference for the formation of products (HI), meaning the reaction is product favored (I). Additionally, since Kc > 1, the equilibrium lies to the right (III), indicating that the forward reaction is favored. Therefore, statements I and III are true, and choice A is the best answer.

The Equilibrium Constant for the Formation of Hydrogen Iodide from Hydrogen