A fixed amount of a real gas is compressed and cooled.

A student investigates the pressure of a fixed amount of gas at constant temperature by changing the volume of the container.

A balloon contains $0.150\ \text{mol}$ of helium at $25.0\ ^\circ\text{C}$ and $1.20\times 10^5\ \text{Pa}$. Assume ideal gas behaviour.

A fixed mass of gas is sealed in a rigid metal cylinder. Its pressure is $1.01\times 10^5\ \text{Pa}$ at $20.0\ ^\circ\text{C}$. The cylinder is warmed to $60.0\ ^\circ\text{C}$.

A fixed amount of an ideal gas was kept at constant temperature while the volume of the container was changed. The graph shows the measured pressure at each volume, with one point labelled A.

Different gases were measured at standard temperature and pressure, STP. The table shows the amount of gas and the volume occupied by each sample.

A volatile liquid is vaporized and the gas is collected over water. The mass of liquid vaporized is $0.108\ \text{g}$. The gas volume is $4.86\times 10^{-5}\ \text{m}^3$ at $296\ \text{K}$. The total pressure is $1.012\times 10^5\ \text{Pa}$ and the water vapour pressure at $296\ \text{K}$ is $2.80\times 10^3\ \text{Pa}$.

An impure sample of calcium carbonate decomposes on heating according to the equation:

$\text{CaCO}_3(s)\to \text{CaO}(s)+CO_2(g)$

A $0.842\ \text{g}$ sample produces $1.68\times 10^{-4}\ \text{m}^3$ of $CO_2$ at $298\ \text{K}$ and $1.00\times 10^5\ \text{Pa}$. Assume ideal gas behaviour.

Ammonia, $NH_3$, and nitrogen, $N_2$, are compared under the same conditions of $250\ \text{K}$ and $5.00\times 10^5\ \text{Pa}$.

A rigid vessel of volume $2.50\times 10^{-3}\ \text{m}^3$ contains $0.0300\ \text{mol}$ of argon at $298\ \text{K}$. A further $0.0100\ \text{mol}$ of argon is added and the vessel is then heated to $350\ \text{K}$. Assume ideal gas behaviour.

The compressibility factor, $Z$, is equal to $PV/(nRT)$. For an ideal gas, $Z=1$. The table shows values of $Z$ for nitrogen at different temperatures and pressures.

Oxygen gas was collected in a gas syringe during the decomposition of hydrogen peroxide. The table shows the final gas volume and the conditions in the laboratory.

A gas sample in a sealed piston was changed from state 1 to state 2. The diagram gives the pressure, volume and temperature for state 1, and the volume and temperature for state 2.

A fixed amount of gas was sealed in a rigid container. The pressure was recorded at different temperatures. The graph shows pressure plotted against temperature in degrees Celsius.

Students used measured values of pressure, volume, amount and temperature for an ideal gas to calculate the gas constant, $R$. The table and plot show their results from several trials.

The graph shows pressure against temperature for a fixed amount of gas in a container of constant volume. The ideal prediction and experimental results for a real gas are shown.

A student determines the molar volume of hydrogen gas by reacting magnesium with excess hydrochloric acid and collecting the hydrogen in a gas syringe. A $0.0450\ \text{g}$ strip of magnesium produces $4.50\times 10^{-5}\ \text{m}^3$ of hydrogen at room temperature and pressure.

$\text{Mg}(s)+2HCl(aq)\to \text{MgCl}_2(aq)+H_2(g)$

A gas was collected over water and used to determine the molar mass of a volatile compound. The table shows the experimental data. The total pressure is the pressure of the dry gas plus the pressure of water vapour.

The table shows compressibility factors for methane, carbon dioxide and ammonia under comparable conditions. An ideal gas has $Z=1$.

The molar mass of a volatile liquid was determined by vaporizing it in a flask of known volume. The apparatus and data are shown.

A fixed amount of gas was compressed at constant temperature. The data were processed by plotting pressure against the reciprocal of volume, $1/V$. The best-fit line has a gradient shown on the graph.

A student reacts $0.0400\ \text{g}$ of magnesium ribbon with excess dilute hydrochloric acid and collects the hydrogen gas in a gas syringe. The collected gas is saturated with water vapour at $25.0\ ^\circ\text{C}$. The atmospheric pressure is $101.2\ \text{kPa}$. The vapour pressure of water at this temperature is $2.8\ \text{kPa}$.

A fixed amount of gas is placed in a sealed syringe at $300\ \text{K}$. The pressure is measured at different volumes.

A sealed metal aerosol can contains a fixed amount of propellant gas. At $20.0\ ^\circ\text{C}$ the gas pressure inside the can is $100\ \text{kPa}$. The can volume is constant.

Helium, carbon dioxide and ammonia are stored separately in identical cylinders at the same temperature and pressure. The cylinders are then cooled and compressed.

A fixed amount of gas in a rigid metal flask was cooled. The graph compares the measured pressure with the pressure predicted by the ideal gas equation.

A volatile liquid is vaporized in a sealed $125\ \text{cm}^3$ flask at $100.0\ ^\circ\text{C}$. After cooling, the mass of condensed liquid in the flask is found to be $0.246\ \text{g}$. The pressure of the vapour before cooling is $100.5\ \text{kPa}$.

A sample of impure calcium carbonate is reacted with excess hydrochloric acid. The carbon dioxide produced is collected and measured at $25.0\ ^\circ\text{C}$ and $101\ \text{kPa}$. A $2.50\ \text{g}$ sample produces $0.510\ \text{dm}^3$ of carbon dioxide.

A gaseous hydrocarbon is collected over water to determine its molar mass. The mass of gas collected is $0.134\ \text{g}$, the gas volume is $58.0\ \text{cm}^3$, the temperature is $25.0\ ^\circ\text{C}$ and the total pressure is $101.6\ \text{kPa}$. The vapour pressure of water at $25.0\ ^\circ\text{C}$ is $3.17\ \text{kPa}$.

In an experiment, carbon dioxide is generated and collected in a $250.0\ \text{cm}^3$ gas syringe at constant temperature. At RTP, one mole of gas occupies $24.0\ \text{dm}^3\ \text{mol}^{-1}$. A graph of mass lost by the reaction flask against gas volume is used to determine the molar mass of the gas.

Sodium azide, $NaN_3$, can decompose rapidly to form sodium and nitrogen gas in an inflator. The simplified equation is:

$2NaN_3(s)\to2Na(s)+3N_2(g)$

A sealed test chamber of volume $12.0\ \text{dm}^3$ contains nitrogen produced by decomposing $5.00\ \text{g}$ of sodium azide. The gas temperature immediately after decomposition is $450\ \text{K}$.

A $600\ \text{cm}^3$ sample of the mixture decreases to $420\ \text{cm}^3$ after treatment with excess aqueous potassium hydroxide. Carbon dioxide is removed completely by passing the mixture through excess aqueous potassium hydroxide. All gas volumes are measured at the same temperature and pressure unless stated otherwise.

The quantity $PV/(nRT)$ is equal to $1.00$ for an ideal gas. A student measures this quantity for two real gases at $298\ \text{K}$ as pressure is increased. The plotted values are hypothetical gas-phase data used to illustrate deviation from ideal behaviour.

A student uses a computer simulation to investigate a fixed amount of ideal gas. The simulation can hold either pressure, volume or temperature constant while the other variables are changed.