Question

4. At 500.0 K, gaseous NOCI decomposed to NO and Cl2 according the following reaction: 2NOCI(g) = 2NO(g) + Cl2(g) If 1.00 mole of NOCI is placed in a 1.00 liter contained, and at equilibrium, the concentration is 0.91M, what is the equilibrium constant, Kc? Initial Change Equilibrium

At 500.0 K, gaseous NOCl decomposed to NO and Cl2 according the following reaction:

2NOCl(g) ⇌ 2NO(g) + Cl2(g)
If 1.00 mole of NOCl is placed in a 1.00 liter contained, and at equilibrium, the

concentration is 0.91M, what is the equilibrium constant, Kc?

Answer 1

Molarity is the number of moles of solute present in one litre of solution.

M = Number of moles of solute/Volume of solution in Litres

Initial concentration of NOCl = [NOCl]

= 1 mole/ 1 L = 1 M

Let the "x" is the change in concentration of NOCl.

IN POTTEETTITY 2 No cl (g) 2 NO (g) + Cl2 lg) K - [Nole [clale Nocl] Given that [Nocle = 0.91M 2 NOCI ( 1) = 2 NO(g) + Cl2 (5) 0 ta Initial change Equilibrium - N ta Cai Since e nocll. = 1-X=0.91M ge=0.09M .: Creole = 0.09 m [ca] = 2 = 0.09M 0.09M 0 0.045M. 2 i. Kas 10.09) rx (0.0455) M (0.91M) ~ 0.0004402 = 4.402 X104 M