IB Chemistry HL 1.5.3 Molar Volume Questions

Relate equal gas volumes at the same temperature and pressure to equal amounts, then use balanced-equation volume ratios and molar volume at STP/SATP.

Exam points

Convert between gas amount and volume using the molar volume stated for the temperature and pressure conditions.
Compare gas pressure, volume and temperature using absolute-temperature and fixed-mass relationships.
Interpret pressure–volume or volume–temperature graphs for a fixed mass of gas and identify the quantities held constant.

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Study 1.5.3—Molar volume conceptsOpen the corresponding Concept lesson for explanations, examples and exam connections.

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Two hydrides of nitrogen are ammonia and hydrazine, $\mathrm{N}_{2} \mathrm{H}_{4}$ . One derivative of ammonia is methanamine whose molecular structure is shown below.

Figure for Question IB Chemistry HL 1.5.3 Molar Volume Questions question 1 — IB Chemistry HL

Calculate, showing your working, the mass of hydrazine needed to remove all the dissolved oxygen from $1000 \mathrm{dm}^{3}$ of the sample.

Calculate the volume, in $\mathrm{dm}^{3}$ , of nitrogen formed under SATP conditions.
(The volume of 1 mol of gas $=24.8 \mathrm{dm}^{3}$ at SATP.)

$n(\mathrm{N}_{2}\mathrm{H}_{4})=n(\mathrm{O}_{2}) =\frac{8.0\ \mathrm{g}}{32.00\ \mathrm{g\ mol^{-1}}} =0.25\ \mathrm{mol}$ $\text{volume of nitrogen} =0.25\ \mathrm{mol}\times24.8\ \mathrm{dm^{3}\ mol^{-1}} =6.2\ \mathrm{dm^{3}}$

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IB Chemistry HL 1.5.3 Molar Volume Questions question 1