At 100 C, the following two reactions have the denoted equilibrium constants.
2NO(g) + Br ₂(g) 2NOBr(g) K=2.4
Br²(g) + Cl2(g) 2BrCl(g) K=7.5
What is the value of the equilibrium constant for the reaction?
2NOBr(g) + C_l2(g) $\leftrightarrows$ 2NO(g) + 2BrCl(g)

Question

At 100 C, the following two reactions have the denoted equilibrium constants.
2NO(g) + Br ₂(g) 2NOBr(g) K=2.4
Br²(g) + Cl2(g) 2BrCl(g) K=7.5
What is the value of the equilibrium constant for the reaction?
2NOBr(g) + C_l2(g)

\leftrightarrows

2NO(g) + 2BrCl(g)

Quizplus · Accepted Answer

The equilibrium constant for the given reaction can be calculated by multiplying the equilibrium constants of the two reactions that make up the given reaction. Therefore, the equilibrium constant for the given reaction is K = 2.4 * 7.5 = 18.

At 100 C, the Following Two Reactions Have the Denoted ⇆\leftrightarrows ⇆

At 100 C, the Following Two Reactions Have the Denoted $\leftrightarrows$