Question

The equilibrium 2NO(g) + Cl2(g) ⇌ 2NOCl(g) is established at 500 K. An equilibrium mixture of the three gases has partial pressures of 0.0952 atm, 0.171 atm, and 0.281 atm for NO, Cl2, and NOCl, respectively. Calculate the Kp for the reaction using the partial pressures given. Calculate the Kc for this reaction at the same temperature.

Name: the equilibrium 2nog cl2g 2noclg is established at 500 k an equilibrium mixture of the three gases has partial pressures of 00952 atm 0171 atm and 0281 atm for no cl2 and nocl respectively c 28866
Uploaded: 2023-01-24T05:47:40-08:00
Duration: 1 min 13 s
Channel: Sri K
Description: the equilibrium 2nog cl2g 2noclg is established at 500 k an equilibrium mixture of the three gases has partial pressures of 00952 atm 0171 atm and 0281 atm for no cl2 and nocl respectively c 28866

          The equilibrium 2NO(g) + Cl2(g) ⇌ 2NOCl(g) is established at 500 K. An equilibrium mixture of the three gases has partial pressures of 0.0952 atm, 0.171 atm, and 0.281 atm for NO, Cl2, and NOCl, respectively. 
Calculate the Kp for the reaction using the partial pressures given. 
Calculate the Kc for this reaction at the same temperature.

Added by Brittany M.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

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Solved by Expert Sri K

01/24/2023

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314 x 10-5 M-1. Show more…

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The equilibrium 2NO(g) + Cl2(g) ⇌ 2NOCl(g) is established at 500 K. An equilibrium mixture of the three gases has partial pressures of 0.0952 atm, 0.171 atm, and 0.281 atm for NO, Cl2, and NOCl, respectively. Calculate the Kp for the reaction using the partial pressures given. Calculate the Kc for this reaction at the same temperature.