Question

Calculate the value of the equilibrium constant KP for the reaction 2NO(g)+Cl2(g)⇌2NOCl(g) from these equilibrium pressures: NO, 0.050 atm; Cl2, 0.30 atm; NOCl, 1.2 atm.

a) 0.10
b) 0.20
c) 0.50
d) 1.0

Answer 1

The value of the equilibrium constant KP for the reaction 2NO(g) + Cl2(g) ⇌ 2NOCl(g) given the equilibrium pressures is calculated to be approximately 1.0 atm-1, making the correct answer option d.

Step-by-step explanation:

To calculate the value of the equilibrium constant KP for the reaction 2NO(g) + Cl2(g) ⇌ 2NOCl(g), we need to use the given equilibrium pressures. The equilibrium constant KP is defined for gaseous reactions at constant temperature and is given by:

KP = (PNOCl^2) / (PNO^2 ⋅ PCl2)

Substituting the given equilibrium pressures into this equation:

KP = (1.2 atm)^2 / ((0.050 atm)^2 ⋅ 0.30 atm)

KP = 1.44 atm2 / (0.0025 atm2 ⋅ 0.30 atm)

KP = 1.44 atm2 / 0.00075 atm3

KP = 1920 atm-1

The closest answer to this calculated equilibrium constant is d) 1.0 atm-1 (rounded to one significant digit). Thus, option d is the correct answer.