A rigid flask contains argon gas at a pressure of $1.20\times10^5\ \text{Pa}$, a volume of $2.40\times10^{-3}\ \text{m}^3$ and a temperature of $300\ \text{K}$.

A student investigates a fixed mass of gas in a syringe. The temperature is kept constant. The student records the pressure for different volumes.

A fixed amount of gas in a sealed syringe has an initial pressure of $100\ \text{kPa}$, volume of $32\ \text{cm}^3$ and temperature of $290\ \text{K}$. It is compressed to $20\ \text{cm}^3$ and its temperature becomes $330\ \text{K}$.

The same sample of carbon dioxide is tested in two different situations: situation X is at low pressure and high temperature, and situation Y is at high pressure and low temperature.

A sample of helium may be treated as an ideal monatomic gas. The amount of helium is $0.080\ \text{mol}$. Its temperature increases from $22\ ^\circ\text{C}$ to $82\ ^\circ\text{C}$.

A gas is contained in a cubical box. A molecule rebounds elastically from one wall of the box.

A sealed cylinder contains air beneath a movable piston. A force sensor measures the normal force exerted by the gas on the piston while the gas pressure is varied slowly at constant temperature.

A fixed mass of air is compressed slowly in a syringe. The temperature of the air is kept constant by allowing time for thermal equilibrium after each change of volume.

A fixed amount of gas in a flexible sealed container changes from state 1 to state 2. The gas is allowed to reach thermal equilibrium in each state.

Air in a room is modelled as an ideal gas. The pressure is $1.01\times10^5\ \text{Pa}$ and the density is $1.15\ \text{kg m}^{-3}$.

An ideal monatomic gas in a cylinder has pressure $2.0\times10^5\ \text{Pa}$ and volume $1.5\times10^{-3}\ \text{m}^3$.

The pressure-volume diagram shows a cycle for a fixed mass of ideal gas. During the process A to B, the gas expands at a constant pressure of $1.2\times10^5\ \text{Pa}$ from $2.0\times10^{-3}\ \text{m}^3$ to $5.0\times10^{-3}\ \text{m}^3$. During B to C the volume is constant and the pressure decreases. The cycle is completed by C to A.

Nitrogen gas is stored in two containers. Container A is at $8.0\ \text{MPa}$ and $290\ \text{K}$. Container B is at $100\ \text{kPa}$ and $500\ \text{K}$.

A student adds measured amounts of helium to a rigid flask of known volume. The flask is kept in a water bath at constant temperature. The pressure is recorded after each addition.

A gas column is trapped in a narrow capillary tube by a small drop of oil. The capillary is placed in a water bath. The pressure of the trapped gas is constant and the length of the gas column is measured at different temperatures.

A fixed amount of ideal gas undergoes the changes shown on a pressure-volume diagram.

The internal energy of a sample of ideal monatomic gas is measured at different temperatures. The amount of gas is constant.

A molecular simulation of an ideal gas records the number of particles, pressure, volume and temperature for several equilibrium states.

Neon atoms in an ideal gas sample have mass $3.35\times10^{-26}\ \text{kg}$ per atom. The thermodynamic temperature of the gas is $400\ \text{K}$.

A computer model represents an ideal gas in a cubic container. The density and root mean square speed of the molecules are recorded for different states of the gas.

The graph shows how the compressibility factor $Z$ varies with pressure for a real gas at two different temperatures. For one mole of gas, $Z=\dfrac{PV}{RT}$.

A fixed volume of gas is heated in a water bath. A pressure sensor records gauge pressure, which is the pressure above atmospheric pressure. Atmospheric pressure is $101\ \text{kPa}$.

A sealed syringe contains air that may be modelled as an ideal gas. The syringe is placed in a water bath and the plunger is slowly moved so that the air remains in thermal equilibrium with the bath.

A student investigates the pressure law using a fixed mass of gas in a rigid flask of volume $2.40\times10^{-3}\ \text{m}^3$. The flask is placed in water baths at different temperatures. The measured pressure of the gas is plotted against temperature in degrees Celsius.

A sample of neon gas contains $0.150\ \text{mol}$ of atoms. Neon may be treated as an ideal monatomic gas. The temperature of the gas is increased from $290\ \text{K}$ to $410\ \text{K}$.

A simulation gives the distribution of molecular speeds for the same ideal gas at two different temperatures. Vertical markers indicate the root mean square speed for each distribution.

A container of helium is at room temperature. Helium may be modelled as an ideal monatomic gas. The density of the helium is $0.164\ \text{kg m}^{-3}$ and the pressure is $1.00\times10^5\ \text{Pa}$.

The same fixed amount of an ideal gas is taken through three separate processes starting from the same initial state. Process X is at constant temperature, process Y is at constant pressure, and process Z is at constant volume.

A diver releases a small bubble of air at a depth where the absolute pressure is $3.2\times10^5\ \text{Pa}$ and the water temperature is $6^\circ\text{C}$. Near the surface the absolute pressure is $1.0\times10^5\ \text{Pa}$ and the water temperature is $20^\circ\text{C}$. The initial bubble volume is $1.6\ \text{cm}^3$. Assume the amount of gas in the bubble is constant.

A cubic container of side $0.250\ \text{m}$ contains nitrogen gas at $300\ \text{K}$ and pressure $1.20\times10^5\ \text{Pa}$. Nitrogen may be treated as an ideal gas with molar mass $2.80\times10^{-2}\ \text{kg mol}^{-1}$.

Two sealed containers have the same volume and are at the same temperature. Container A holds an ideal gas. Container B holds a real gas close to condensation.

A steel cylinder of volume $12.0\ \text{L}$ contains oxygen gas at $18.0^\circ\text{C}$ and a pressure of $8.00\times10^5\ \text{Pa}$. Oxygen has molar mass $3.20\times10^{-2}\ \text{kg mol}^{-1}$.

A research balloon is filled with helium before launch. At launch the helium volume is $4.8\ \text{m}^3$, the temperature is $288\ \text{K}$ and the pressure is $1.01\times10^5\ \text{Pa}$. At high altitude the pressure is $2.5\times10^4\ \text{Pa}$ and the temperature is $235\ \text{K}$. The balloon material allows the helium to expand without significant leakage until this altitude.

A cylinder contains an ideal monatomic gas fitted with a frictionless piston. The gas is heated slowly at constant pressure and expands from $2.0\times10^{-3}\ \text{m}^3$ to $5.0\times10^{-3}\ \text{m}^3$. The pressure is $1.5\times10^5\ \text{Pa}$ throughout the expansion.

A fixed amount of ideal gas is taken through a cyclic process represented on a pressure-volume diagram. The cycle consists of a constant-volume pressure increase, a constant-pressure expansion, and a compression back to the starting state.