Question

5. 2.00 mol each of SO2 and NO2 are introduced into a 1.00 L reactor at 300°C where Kp = 3.4. SO2(g) + NO2(g) <=> SO3(g) + NO(g) a) Give the general expression for K, for this system in terms of the concentrations ci b) Give the general expression for Kp for this system in terms of the partial pressures Pi. c) Assuming that the gases all behave ideally what is the relationship between K, and Kp? d) What is the equilibrium concentration of all the species? [E = 1.3]

Answer 1

SO₂(g) + NO₂(g) $\leftrightharpoons$ SO₃(g) + NO(g)

(a)

K_c = [SO₃][NO]/([SO₂][NO₂])

(b)

K_P = P_SO3 ×P_NO/(P_SO2 × P_NO2)

(c)

K_p = K_c ×(RT)^∆n_g

∆n_g = 1+1 -( 1+1) = 0

K_P = K_c

(d)

V = 1.00L , let x mol/L concentration of products formed .

K_c = 3.4 = x.x/((2.00-x)(2.00-x))

x/(2.00-x) = √3.4 = 1.8439

x = 1.2967 M

Answers :

[SO₃] = x = 1.30 M

[NO] = x = 1.30 M

[SO₂] = 2.00 - x = 0.70M

[NO₂] = 2.00-x = 0.70 M