Chemistry · Unit 2 · Intermolecular forces and gases · Intermolecular forces
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Ammonia decomposes at high temperature according to the equation: $$\ce{2NH3(g) -> N2(g) + 3H2(g)}$$ Determine the volume of nitrogen gas produced at standard temperature and pressure (STP) when 8.5 g of ammonia completely decomposes. (Molar mass of ammonia = 17 g mol⁻¹; molar volume at STP = 22.7 dm³ mol⁻¹)
Ammonia gas (NH\(_3\)) is synthesised from nitrogen gas (N\(_2\)) and hydrogen gas (H\(_2\)) according to the balanced equation: \[ N_2(g) + 3H_2(g) \rightarrow 2NH_3(g) \] A reaction vessel at 450 K and 8.50 × 10\(^5\) Pa contains 12.0 g of nitrogen gas that reacts completely with excess hydrogen gas. (a) Apply the ideal gas equation to calculate the volume, in litres, occupied by the 12.0 g of nitrogen gas under these conditions. (2 marks) (b) Calculate the mass, in grams, of ammonia gas produced when all the nitrogen reacts. (2 marks)