When nitrogen dioxide (NO2) from car exhaust combines with water in the air, it

Question

When nitrogen dioxide (NO2) from car exhaust combines with water in the air, it forms nitric acid (HNO3), which causes acid rain, and nitrogen oxide; 3NO2(g)+H20(l)-->2HNO3(aq)+NO(g). a) How many molecules of NO2 are needed to react with 0.250 mol of H2O? b) How many grams of HNO3 are produced when 60.0 g of NO2 completly reacts? c) How many grams of HNO3 can be produced if 225 g of NO2 is mixed with 55.2 g of H2O?

Explanation / Answer

NO2(g)+H20(l)-=========>2HNO3(aq)+NO(g). a) How many molecules of NO2 are needed to react with 0.250 mol of H2O? 0.250 mol H2O * (1 mol NO2/1 mol NO2)*(6.022*10^23 molecule of NO2/1 mol NO2) 1.51*10^24 molecule of NO2 b) How many grams of HNO3 are produced when 60.0 g of NO2 completly reacts? 60.0g NO2 (1 mol NO2/46g NO2)*(2 mol HNO3/1 mol NO2)*(63 g HNO3/1 mol HNO3) 164.35 g HNO3 c) How many grams of HNO3 can be produced if 225 g of NO2 is mixed with 55.2 g of H2O? Moles = mass/molar mass Moles of NO2 = 225g/46g/mol = 4.89 mol NO2 Moles of H2O = 55.2g/18g/mol = 3.07 mol H2O The molar ratio is 1 NO2(g) : 1H20(l) So H2O is the limiting reagent 3.7 mol H2O*(2 mol HNO3/1 mol H2O)*(63 g HNO3/1 mol HNO3) 386.82 g of HNO3

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