Please solve F.

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 with4mol of hydrogen. How many moles of oxygen are needed to "use up" all of the hydrogen? How many moles of water molecules are produced? nof O₂= 2 nof H₂O = 4 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.) |E_chem| = kJ 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? There is a net ---Select--- input release of energy, and the chemical energy ---Select--- increases decreases . D. Assume this reaction takes place inside a thermally insulated container with immovable walls. If the chemical energy is increasing, explain where that energy comes from. If the chemical energy is decreasing, explain where that energy goes. Be specific and thoroughly explain your reasoning.

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E. Predict what will happen to the temperature (i.e., whether it will increase, decrease, or stay the same) and explain how you can tell.

Score:2 out of 2

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F. If the system was at 300 K before the reaction took place, what is the final temperature after the reaction? T_f= K