Please answer E, F, H, and L

I will rate for responses.

S1. Many chemists thought that the direct combination of nitrogen with hydrogen was impossible, but in 1905 the German chemist Fritz Haber (1868-1934) showed that the reaction actually occurs under certain conditions.

a) Write a balanced equation and the equilibrium constant expression for the reaction between nitrogen gas, N2, and hydrogen gas, H2, to form ammonia, NH3.

b) Hydrogen and nitrogen are combined in a 1.0-L reaction vessel, and the system comes to equilibrium at 472 C. The equilibrium mixture of gases was analyzed and found to contain 0.1207 M H2, 0.0402 M N2, and 0.00272 M NH3. From these data calculate the equilibrium constant, Kc, for the reaction between hydrogen and nitrogen.

c) The concentrations of products and reactants can also be expressed in terms of partial pressure in bar. What is the equilibrium constant in terms of partial pressures, Kp?

d) If the equilibrium constants are constant for a given reaction, explain why are Kp and Kc different?

e) Calculate the standard change in Gibbs energy, Go, using Kp for the process of producing ammonia from the equilibrium constant for this reaction at 472 C.

f) If you allow the mixture to expand into a second 1.0-L evacuated reaction vessel (so that the total volume the reaction mixture can explore is 2.0-L) and come to equilibrium at 472 C, what is the change in Gibbs energy, G, for the process that occurs?

g) What does your answer in f) tell you about the spontaneous direction of the reaction as the volume increases?

h) Calculate the standard change in Gibbs energy for the reaction, Go r, for the reaction at 298.15 K from the standard free energies of formation, Go f, of the products and reactants.

i) Do you expect the reaction to increase, decrease, or not change the entropy of the system? Briefly explain your answer.

j) Would you expect the reaction to be endothermic or exothermic? Briefly explain your answer. k) Calculate the equilibrium constant, Kp, for this reaction at 298.15 K.

l) Calculate the standard enthalpy and the entropy of the balanced reaction at 298.15 K. Are the answers consistent with your predictions in i) and j)?

m) Suggest 2 different ways to increase the amount of ammonia produced by this reaction, and explain your answers.