2SO2(g) + O2(g) <--> 2SO3(g) A sealed reaction vessel is charged with 5.0 atm SO2 and...

2SO2(g) + O2(g) <--> 2SO3(g)

A sealed reaction vessel is charged with 5.0 atm SO2 and 2.5 M atm at 500 degrees Celsius. The reaction is allowed to equilibriate. At equilibrium 3.0 atm of SO3 is produced. What is the equilibrium concentration of each species. What is Kc for this reaction? Show all work.

Expert Solution

Initial 5.0 2.5 0

Final (5.0-2x) (2.5-x) 2x

Since the pressure of SO3 = 3 atm at equilibrium, hence the value of x=1.5 atm

Pressure of [SO2] = 5.0 - 2(1.5) = 2 atm

Pressure of [O2] = 2.5 - 1.5 = 1 atm

Kp = [SO3]^2/[SO2]^2[O2] = (3)^2/(2)^2 = 9/4 = 2.25

Kp = Kc(RT)^{change in moles )

change in moles = 2 - (1+2) = -1

Kc = Kp(RT) = 2.25 * 0.0821 * (273+500) = 142.79

queen_honey_blossom answered 2 years ago

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