consider the reaction 2H2(g) + O2(g) → 2H2O(g). The following bond energies have been determined experimentally: H-H 436 kJ/mol O=O 497 kJ/mol H-O 464 kJ/mol A. Suppose we start with 4 mol of hydrogen. How many moles of oxygen are needed to "use up" all of the hydrogen? How many moles of water molecules are produced? B. For the number of moles in part A, what is the difference in chemical energy between the reactants and the products for this reaction? (Give the absolute value only.) C. Does your answer to part B represent a net input of energy, or a net release of energy if the reaction proceeds in the direction indicated? Does the chemical energy increase, or decrease? E. If the system was at 300 K before the reaction took place, what is the final temperature after the reaction?