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5 March, 12:30

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?

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  1. 5 March, 14:33
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    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
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