Question

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

Name: at 35oc the equilibrium constant for the reaction 2noclg 2nog cl2g is kc 16 105 an equilibrium mixture was found to have the following concentrations of cl2 and nocl cl2 12 102 m nocl 28 101 90249
Uploaded: 2022-07-13T22:48:22-08:00
Duration: 1 min 12 s
Channel: Ronald Prasad
Description: at 35oc the equilibrium constant for the reaction 2noclg 2nog cl2g is kc 16 105 an equilibrium mixture was found to have the following concentrations of cl2 and nocl cl2 12 102 m nocl 28 101 90249

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

Added by Robert F.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Ronald Prasad

07/13/2022

Step 1

Step 1: Write the equilibrium expression for the reaction: \[ K_c = \frac{[NO]^2[Cl_2]}{[NOCl]^2} \] Show more…

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