N2 (g) + 2O2 (g) + 2 NO2 (g)

3NO2 (g) + H2O (g) = 2HNO3 (aq) + NO (g)

a. a car burns 4.00 x 10^2 g of N2. How many grams of HNO3 will be produced?

b. what is the minimum amount of O2 needed in grams?

a) 1201.6 grams of HNO3 is produced

b) The minimum amount of O2 is 915.2 grams

Explanation:

Step 1: Data given

Mass of N2 = 400 grams

Molar mass N2 = 28.0 g/mol

Step 2: The balanced equation

N2 (g) + 2O2 (g) → 2 NO2 (g)

3NO2 (g) + H2O (g) → 2HNO3 (aq) + NO (g)

Step 3: Calculate moles N2

Moles N2 = mass N2 / molar mass N2

Moles N2 = 400 grams / 28.0 g/mol

Moles N2 = 14.3 moles

Step 4: Calculate moles O2

For 1 mol N2 we need 2 moles O2 to produce 2 moles NO2

For 14.3 moles N2 we need 28.6 moles O2 to produce 28.6 moles NO2

Step 5: Calculate mass O2

Mass O2 = moles O2 * molar mass O2

Mass O2 = 28.6 moles * 32.0 g/mol

Mass O2 = 915.2 grams

Step 6: Calculate moles NO2

For 14.3 moles N2 we need 28.6 moles O2 to produce 28.6 moles NO2

Step 7: Calculate moles HNO3

For 3 moles NO2 we need 1 moles H2O to produce 2 moles HNO3 and 1 mol NO

For 28.6 moles NO2 we need 2/3 * 28.6 = 19.07 moles HNO3

Step 8: Calculate mass HNO3

Mass HNO3 = moles HNO3 * molar mass HNO3

Mass HNO3 = 19.07 g/mol * 63.01 g/mol

Mass HNO3 = 1201.6 grams

1201.6 grams of HNO3 is produced