If the system below is at equilibrium in a closed vessel and a small amount of nitrous acid is added, what would be expected to happen? HN3(l) 2 H2O(l) <--> N2H4(l) + HNO2(l) ?Hº = +641 kJ Question 2 options: a. Some HN3 would be used up in re-establishing equilibrium b. Some HNO2 would be formed in re-establishing equilibrium c. Some HNO2 would be formed, and some N2H4 would be lost d. More HN3 and H2O would be formed e. The temperature would decrease, and the forward reaction would be favored