The equilibrium constant for the reaction of bromine with chlorine to form bromine monochloride is 58.0 at a certain temperature. Br₂(g) + Cl₂(g) 2BrCl(g)
What is the equilibrium constant for the following reaction?
BrCl(g) ½Br₂(g) + ½Cl₂(g)

Question

The equilibrium constant for the reaction of bromine with chlorine to form bromine monochloride is 58.0 at a certain temperature. Br₂(g) + Cl₂(g)

The equilibrium constant for the reaction of bromine with chlorine to form bromine monochloride is 58.0 at a certain temperature. Br<sub>2</sub>(g) + Cl<sub>2</sub>(g) 2BrCl(g) What is the equilibrium constant for the following reaction? BrCl(g) ½Br<sub>2</sub>(g) + ½Cl<sub>2</sub>(g) A) 2.97 × 10<sup>-4</sup> B) 1.72 × 10<sup>-2</sup> C) 3.45 × 10<sup>-2</sup> D) 1.31 × 10<sup>-1</sup> E) > 1.00

2BrCl(g)
What is the equilibrium constant for the following reaction?
BrCl(g)

½Br₂(g) + ½Cl₂(g)

Quizplus · Accepted Answer

The Answer of The equilibrium constant for the reaction of bromine with chlorine to form bromine monochloride is 58.0 at a certain temperature. Br₂(g) + Cl₂(g) 2BrCl(g) What is the equilibrium constant for the following reaction? BrCl(g) ½Br₂(g) + ½Cl₂(g)

The Equilibrium Constant for the Reaction of Bromine with Chlorine