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The formation of nitrogen oxide, NO, from N2(g) and O2(g),
Chapter 6, Problem 121CQ(choose chapter or problem)
The formation of nitrogen oxide, NO, from N2(g) and O2(g), requires 21.6 kcal of heat. (6.9)N2(g) + O2(g) ? 2NO(g) ?H = + 21.6 kcala. How many kilocalories are required to form 3.00 g of NO?b. What is the complete equation (including heat) for the decomposition of NO?c. How many kilocalories are released when 5.00 g of NO decomposes to N2 and O2
Questions & Answers
QUESTION:
The formation of nitrogen oxide, NO, from N2(g) and O2(g), requires 21.6 kcal of heat. (6.9)N2(g) + O2(g) ? 2NO(g) ?H = + 21.6 kcala. How many kilocalories are required to form 3.00 g of NO?b. What is the complete equation (including heat) for the decomposition of NO?c. How many kilocalories are released when 5.00 g of NO decomposes to N2 and O2
ANSWER:Solution 121CQStep 1 of 3:Given reaction:N2(g) + O2(g) 2NO(g) H = + 21.6 kcala. Here, we are asked to find the kilocalories are required to form 3.00 g of NOMolar mass of NO = 30.01 g/molH = + 21.6 kcal1 mol of NO = 30.01 g of NO. So, the mole-mass factor is: and In the reaction we see, there are 2 moles of NO and it is equal to H = + 21.6 kcal. So, the factor is: and Thus, the energy in kilocalories is: = 3.00 g NO = 1.079 kcalHence, the kilocalories are required to form 3.00 g of NO is 1.079 kcal.________________