A sample of magnesium nitride (Mg3N2\text{Mg}_3\text{N}_2Mg3N2) was reacted completely with water to produce ammonia gas, NH3\text{NH}_3NH3, according to the following equation:
Mg3N2(s)+6H2O(l)→3Mg(OH)2(s)+2NH3(g) \text{Mg}_3\text{N}_2(\text{s}) + 6\text{H}_2\text{O}(\text{l}) \rightarrow 3\text{Mg(OH)}_2(\text{s}) + 2\text{NH}_3(\text{g}) Mg3N2(s)+6H2O(l)→3Mg(OH)2(s)+2NH3(g)The volume of ammonia gas collected was 120.0 cm3 at a temperature of 298 K and a pressure of 98.0 kPa.
What is the amount, in moles, of magnesium nitride that reacted?
The gas constant, R=8.31 J K−1 mol−1R = 8.31\text{ J K}^{-1}\text{ mol}^{-1}R=8.31 J K−1 mol−1
2.37×10−62.37 \times 10^{-6}2.37×10−6
2.37×10−32.37 \times 10^{-3}2.37×10−3
4.75×10−34.75 \times 10^{-3}4.75×10−3
9.50×10−39.50 \times 10^{-3}9.50×10−3
79 exam-style questions on AQA A Level Chemistry Amount of substance, covering Relative atomic mass and relative molecular mass, The mole and the Avogadro constant, The ideal gas equation, Empirical and molecular formula, and Balanced equations and associated calculations. Each one has a worked solution and a mark scheme showing where the marks go.