How many grams of ammonia must you start with to make 900.00 l of a 0.140 m aqueous solution of nitric acid? assume all the reactions give 100% yield?

You need the set of reactions that goes from ammonia to nitric acid.

1) 4NH3 (g) + 5O2 (g) - - >4NO (g) + 6H2O (g)

2) 2NO (g) + O2 (g) - - >2NO2 (g)

3) 3NO2 (g) + H2O (l) - - >2HNO3 (aq) + NO (g)

State the ratio of moles of HNO3 to NH3:

4 moles of NH3 produce 4 mole of NO,

4 moles of NO produce 4 moles of NO2

4 moles of NO2 produce 4 * (2 / 3) moles of HNO3 = 8/3 moles of HNO3.

=> (8/3) moles HNO3 : 4 moles NH3

Calculate the number of moles of HNO3 in 900.00 l of 0.140 M solution

M = n / V = > n = M * V = 0.140 M * 900.00 liter = 126 moles HNO3

Use proportions:

(8/3) moles HNO3 / 4 moles NH3 = 126 moles HNO3 / x

=> x = 126 moles HNO3 * 4 moles NH3 / (8/3 moles HNO3) = 189 moles NH3

Convert moles to grams:

molar mass NH3 = 14 g/mol + 3 * 1g/mol = 17 g/mol

mass in grams = number of moles * molar mass = 189 moles * 17 g/mol = 3213 g

Answer: 3213 g.