Sodium azide (NaN3\text{NaN}_3NaN3) is used in automobile airbags to rapidly inflate them during a collision. When triggered, it undergoes extremely rapid thermal decomposition to release nitrogen gas according to the following equation:
2NaN3→2Na+3N2 2\text{NaN}_3 \rightarrow 2\text{Na} + 3\text{N}_2 2NaN3→2Na+3N2Calculate the mass, in grams, of nitrogen gas (N2\text{N}_2N2) that would be produced by completely decomposing 13.0 g13.0\text{ g}13.0 g of sodium azide. [MrM_rMr of NaN3=65\text{NaN}_3 = 65NaN3=65]
mass of nitrogen gas = _______________ g\text{g}g
Use your answer from part (a) to calculate the volume, in cm3\text{cm}^3cm3, at room temperature and pressure, of nitrogen gas that would be produced by completely decomposing 13.0 g13.0\text{ g}13.0 g of sodium azide.
Assume one mole of nitrogen gas has a volume of 24 000 cm324\,000\text{ cm}^324000 cm3 at room temperature and pressure.
volume of nitrogen gas = _______________ cm3\text{cm}^3cm3
80 exam-style questions on Edexcel IGCSE Chemistry Chemical formulae, equations and calculations. Each one has a worked solution and a mark scheme showing where the marks go.