16 aoints: Consider the following equilibrium reaction for this question: N2(g)+3H2(g)2NH3(g) a. Write out a generic expression for K as a function of molarities given the above reaction. b. At 500C, the equilibrium mixture of NH3,H2, and N2 was found to contain 0.412MNH3, 1.35MH2, and 1.15MN2. Calculate the equilibrium constant. c. Calculate the equilibrium for the reverse reaction at 500C:2NH3(g)N2(g)+3H2(g) d. Predict what effect (if any) will increasing the volume of the reaction vessel cause? Answer shift left, right, or no change (no explanation needed). 6. 16 points: Consider the following equilibrium reaction: 4NH3(g)+5O2(g)4NO(g)+6H2O(g)H=904.4kJ/mol a. How does each of the following affect the amount of NO(g) present to re-establish equilibrium? Answer increase, decrease, or no change. i. Adding O2(g) : ii. Decrease temperature: iii. Increase the pressure: iv. Adding liquid water: v. Adding a catalyst: b. Circle true or false: This reaction is exothermic, so it must be fast. c. Circle true or false: Adding a catalyst to this reaction will decrease the H. d. Circle true or false: The reverse reaction as