Use of amount of substance in relation to volumes of gases (chemistry only) (HT only): แบบฝึกหัด

Propane burns in oxygen according to the following balanced equation:
\(C_3H_8(g) + 5O_2(g) \rightarrow 3CO_2(g) + 4H_2O(l)\)

Calculate the volume of oxygen gas required for the complete combustion of \(150\text{ cm}^3\) of propane. Assume all volumes are measured at the same temperature and pressure.

Calculate the volume of carbon dioxide gas produced at room temperature and pressure (RTP) when \(5.0\text{g}\) of calcium carbonate (\(\text{CaCO}_3\)) is completely decomposed by heating.
\(\text{CaCO}_3 \rightarrow \text{CaO} + \text{CO}_2\)
(Relative formula mass: \(\text{CaCO}_3 = 100\); Molar gas volume at RTP = \(24\text{ dm}^3\))

Ammonia is produced in the Haber process via the following reversible reaction:
\(N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)\)

In a closed system, a mixture of \(60\text{ dm}^3\) of nitrogen and \(120\text{ dm}^3\) of hydrogen are reacted. Calculate the maximum volume of ammonia that could be produced, and identify the volume of the gas remaining in excess (assuming the reaction goes to completion and all volumes are measured at the same temperature and pressure).

Calculate the volume of oxygen gas required for the complete combustion of \(5.0\text{ dm}^3\) of butane (\(\text{C}_4\text{H}_{10}\)) at the same temperature and pressure.
\(2\text{C}_4\text{H}_{10} + 13\text{O}_2 \rightarrow 8\text{CO}_2 + 10\text{H}_2\text{O}\)

A student decomposes a sample of potassium chlorate according to the equation:
\(2KClO_3(s) \rightarrow 2KCl(s) + 3O_2(g)\)

If \(1.47\text{ g}\) of potassium chlorate is completely decomposed, calculate the volume of oxygen gas produced at room temperature and pressure (RTP).

(Relative formula mass: \(KClO_3 = 122.5\); Molar gas volume at RTP = \(24\text{ dm}^3\))

Calculate the volume occupied by 0.5 moles of carbon dioxide gas at room temperature and pressure (rtp). Assume the volume of one mole of any gas at rtp is \(24\text{ dm}^{3}\).

When \(8.40\text{ g}\) of magnesium carbonate (\(MgCO_3\)) is heated, it decomposes to form magnesium oxide and carbon dioxide gas according to the equation:
\(MgCO_3(s) \rightarrow MgO(s) + CO_2(g)\)

Calculate the volume of carbon dioxide gas produced at room temperature and pressure (RTP).

(Relative atomic masses: \(Mg = 24, C = 12, O = 16\). Molar gas volume at RTP = \(24\text{ dm}^3\))

At room temperature and pressure (RTP), the volume of one mole of any gas is \(24 \text{ dm}^3\).

Calculate the volume, in \(cm^3\), occupied by \(0.88 \text{ g}\) of carbon dioxide (\(CO_2\)) gas at RTP.

(Relative atomic masses: \(C = 12, O = 16\))

Magnesium reacts with hydrochloric acid to produce magnesium chloride and hydrogen gas:
\(Mg(s) + 2HCl(aq) \rightarrow MgCl_2(aq) + H_2(g)\)

A scientist reacts \(0.12 \text{ g}\) of magnesium with \(50.0 \text{ cm}^3\) of \(0.10 \text{ mol/dm}^3\) hydrochloric acid.

(a) Show by calculation which reactant is the limiting reactant. (4 points)

(b) Calculate the volume of hydrogen gas produced at room temperature and pressure. (2 points)

(Relative atomic masses: \(Mg = 24, H = 1, Cl = 35.5\). Molar gas volume = \(24 \text{ dm}^3\))