At 35 o C, the equilibrium constant for the followingreaction is K c = 1.6 x 10

Question

At 35oC, the equilibrium constant for the followingreaction is Kc = 1.6 x 10-5. 2NOCl(g) <---> 2NO(g) + Cl2(g) An equilibrium mixture was found to have the followingconcentrations of Cl2 and NOCl: [Cl2] = 1.2 x 10-2M; [NOCl] =2.8 x 10-1M. Calculate the concentrationof NO(g) at equilibrium. At 35oC, the equilibrium constant for the followingreaction is Kc = 1.6 x 10-5. 2NOCl(g) <---> 2NO(g) + Cl2(g) An equilibrium mixture was found to have the followingconcentrations of Cl2 and NOCl: [Cl2] = 1.2 x 10-2M; [NOCl] =2.8 x 10-1M. Calculate the concentrationof NO(g) at equilibrium.

Explanation / Answer

The answer is b. If you take my answer to two significantfigures.

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