I need help with both sections A and B. thank you

+(ten marks) Use the following information to answer the next question. In the Haber-Bosch process of manufacturing ammonia, nitrogen is treated with hydrogen, which results in an exothermic reaction. An iron catalyst (Fe3+) is used in the process and aluminum oxide and potassium oxide are used as promoters. The following reactions takes place at 25C: N2(g) + 3H2(g) + 2NH3(g) +92 kJ A. Indicate the direction in which the equilibrium will shift when temperature is increased volume is increased pressure is decreased - a catalyst is added - the concentration of N2(g) is increased helium gas is added at constant volume, so that the total pressure is increased B. A mixture of 0.48 mol of N2(g) and 0.93 mol of H2(g) is used in the above process. A rigid reaction vessel of 10.0 L capacity is used. Calculate the value of the equilibrium constant and the composition of the equilibrium mixture at 25C, if the equilibrium concentration of H2(g) is 0.049 mol/L