10 (a) Nitric acid can be titrated with a solution of ammonia - Edexcel - GCSE Chemistry - Question 10 - 2019 - Paper 1

The salt formed in this reaction is ammonium nitrate, which corresponds to option D.

To calculate the minimum volume of air required, follow these steps:

1. Calculate the moles of NO: The molar mass of NO = N + O = 14 + 16 = 30 g/mol.

   Moles of NO =
   $\frac{1000 g}{30 g/mol} \approx 33.33 \, \text{mol}$

2. Determine the moles of O2 required: According to the reaction, 2 moles of NO react with 1 mole of O2:

   Moles of O2 required = ( \frac{33.33 , \text{mol}}{2} \approx 16.67 , \text{mol} )

3. Calculate the volume of O2 needed: Using the ideal gas law:

   Volume of O2 = moles × volume per mole = ( 16.67 , \text{mol} \times 24 , \text{dm}^3/mol = 400 , \text{dm}^3 )

4. Determine the volume of air needed: Since air contains 20% oxygen by volume, the volume of air required is:

   Volume of air = ( \frac{400 , \text{dm}^3}{0.20} = 2000 , \text{dm}^3 )

Thus, the minimum volume of air required to react with 1000 g of nitrogen oxide is 2000 dm³.