Question

Question 8 1 pts The Haber process for the production of ammonia is the main industrial process of producing ammonia today. Prior to developing this process, ammonia was difficult to produce on an industrial scale. The reaction for the Haber process is: N2(g) + 3H2(g) = 2 NH3(g). Using the following values, determine the equilibrium constant for this reaction at 25°C. Substance AGR°(kJ/mol) N H2 NH3 - 16.4 Enter your answer to three significant figures.

Answer 1

Given:

Gof(N2(g)) = 0.0 KJ/mol

Gof(H2(g)) = 0.0 KJ/mol

Gof(NH3(g)) = -16.4 KJ/mol

Balanced chemical equation is:

N2(g) + 3 H2(g) ---> 2 NH3(g)

ΔGo rxn = 2*Gof(NH3(g)) - 1*Gof( N2(g)) - 3*Gof(H2(g))

ΔGo rxn = 2*(-16.4) - 1*(0.0) - 3*(0.0)

ΔGo rxn = -32.8 KJ

Given:

T= 25.0 oC

= (25.0+273) K

= 298 K

ΔGo = -32.8 KJ/mol

ΔGo = -32800 J/mol

use:

ΔGo = -R*T*ln Kc

-32800 = - 8.314*298.0* ln(Kc)

ln Kc = 13.2388

Kc = 5.617*10^5

Answer: 5.62*10^5