: What amount of heat is released/absorbed when 15.0 g of XH3 are reacted with excess oxygen? (NOTE: This part is graded based on your answer to Question 1. If you update your answer to the previous part, you MUST resubmit this question)
Need help with part 2: heres the entire answer
An important consideration when exploring the use of new fuel sources is to determine the energy gained from the combustion. Other considerations such as environmental impacts are important but outside the scope of this question. In the case of a new fuel one may not know the heat of formation but other thermochemical reactions can be used to solve for the heat of combustion. Consider the following:
A compound XH3 (MM=25.00 g/mol) will burn in the presence of a platinum catalyst to produce XO.
4XH3(g) + 5O2(g) → 4XO(g) + 6H2O(g)
Part 1: What is the heat of reaction at constant pressure in kJ? Use the following thermal equations:
X2(g) + O2(g) → 2XO(g); ΔH = 200.4 kJ
X2(g) + 3H2(g) → 2XH3(g); ΔH = -91.8 kJ
2H2(g) + O2(g) → 2H2O(g); ΔH = -520.2 kJ
Answer: -976 kJ
Part 2: What amount of heat is released/absorbed when 15.0 g of XH3 are reacted with excess oxygen? (NOTE: This part is graded based on your answer to Question 1. If you update your answer to the previous part, you MUST resubmit this question)
0.150 kJ
How to get part 2? Dont understand how to get 0.150 kj as the answer.
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