Question
Consider the combustion of nitrogen monoxide:
NO(g) + ½ O2(g) NO2 (g) ΔH = -56.5 kJ/mol
How much heat would be released by the combustion of 65 g of NO (g)?
I'm so stuck please help
NO(g) + ½ O2(g) NO2 (g) ΔH = -56.5 kJ/mol
How much heat would be released by the combustion of 65 g of NO (g)?
I'm so stuck please help
Answers
Damon
N + O = 14 + 16 = 30 grams / mol
65 / 30 = 0.2 mols of NO
multiply by the Kilojoules / mol
65 / 30 = 0.2 mols of NO
multiply by the Kilojoules / mol