Chemistry - Chemical Equilibrium Question with Solution | TestHub
A container of capacity V L contains an equilibrium mixture that consists of 1 mole of SO2Cl2, 2 moles of SO2 and 1 mole of Cl2 (all as gases). The pressure is 40.53 kPa and temperature is T K. A certain amount ('x' mole) of Cl2(g) is now introduced keeping the pressure and temperature constant, until the equilibrium volume becomes 2V L. The reaction is SO2Cl2(g) ⇌ SO2(g) + Cl2(g). The value of '30x' is
Answer:
Solution:
Pressure = 40.53 kPa = 0.4 atm Total moles = 1 + 2 + 1 = 4
KP = [(2/4)(0.4)][(1/4)(0.4)]/[(1/4)(0.4)], so KP = (0.2)(0.1)/(0.1) = 0.2 atm
New equilibrium: SO2Cl2 = 1 + y, SO2 = 2 - y, Cl2 = 1 + x - y
At constant P and T, volume doubles, so total moles double to 8
(1+y) + (2-y) + (1+x-y) = 8, so x - y = 4 and Cl2 = 5
KP = (0.4/8)(2-y)(5)/(1+y) = 0.2
0.25(2-y) = 0.2(1+y), so 0.3 = 0.45y and y = 2/3
x = 4 + 2/3 = 14/3
30x = 140, written as 0140
