A 22.75 g sample of ICl(g) is placed in a container of capacity 1642 mL and heated to 500 K. The equilibrium pressure of Cl₂(g) in the system is 1.5 atm. The value of K_P for the reaction:
2ICl(g) ⇌ I₂(g) + Cl₂(g) is (Given: Atomic masses: I = 127, Cl = 35.5)

Question

A 22.75 g sample of ICl(g) is placed in a container of capacity 1642 mL and heated to 500 K. The equilibrium pressure of Cl₂(g) in the system is 1.5 atm. The value of K_P for the reaction:

2ICl(g) ⇌ I₂(g) + Cl₂(g) is (Given: Atomic masses: I = 127, Cl = 35.5)

TestHub · Accepted Answer

Moles of ICl = 22.75/162.5 = 0.14 mol Moles of Cl₂ at equilibrium = PV/RT = (1.5)(1.642)/[(0.0821)(500)] = 0.06 mol

I₂ = 0.06 mol and ICl left = 0.14 - 2(0.06) = 0.02 mol

P_ICl = (0.02)(0.0821)(500)/1.642 = 0.5 atm

P_I2 = 1.5 atm

K_P = (P_I2)(P_Cl2)/(P_ICl)² = (1.5)(1.5)/(0.5)²

K_P = 9

Chemistry - Chemical Equilibrium Question with Solution | TestHub

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