Question

Consider the reaction for the Haber Process: 3H_{2 (g)} + N_{2 (g)} <--> 2NH_3(g)

A mixture of 1.0 mol each of N₂, H₂, and NH₃ are placed into a 1.0 L flask and allowed to come to equilibrium at 500.0 C. K_p at this temperature is 1.45 x 10^-5 atm^-2.

A.) What is the value of K_c at this temperature? irst find the relationship between K_c and K_p in terms of RT. Then substitute T = 773K and R = 0.0821 (L x atm)/(mol x k)

(Note that PV=nRT. so P=nRT/V)

B.) Will this reaction proceed towards producte or towards reactants in order to reach equilibrium? Show how you determined your answer.

C.) Represent the equilibrium concentrations of H₂, N₂, and NH₃ in rwema od X, where X is the moles/L of N₂ produced. Substitute these equilibrium concentrations into the equilibrium constant expression.

D.) Solve this expression for X What are the largest and smallest possible values that X can have for this system?

Answer 1

3H_{2 (g)} + N_{2 (g)} <--> 2NH_3(g)

Kp = Kc(RT)n

n = 2-(3+1) = -2

R = 0.0821L-atm/mole-K

Kp = 1.45*10^-5

T   = 773K

Kp = Kc(RT)n

1.45*10^-5 = Kc(0.0821*773)^-2

   Kc           = 1.45*10^-5 *4027.6

                    = 5840.02*10^-5

                   = 0.05840

Qc            = [NH3]^2/[N2][H2]^3

                    = 1^2/1*1^3   = 1

Qc>Kc The equilibrium shift to left side. The reaction proceed towards reactants

c.