B.3 Gas laws

A sample of a gas has volume $V$ and contains $N$ molecules, each of mass $m$. The average translational speed of the molecules is $u$.

Which expression is equivalent to the pressure of the gas?

A.  $\frac{1}{3}\frac{NV}{m}{u}^2$

B.  $\frac{1}{3}\frac{Nm}{V}{u}^2$

C.  $\frac{1}{3}\frac{N}{mV}{u}^2$

D.  $\frac{1}{3}\frac{m}{NV}{u}^2$

A sample of a gas has volume $V$ and contains $N$ molecules, each of mass $m$. The average translational speed of the molecules is $u$.

Which expression is equivalent to the pressure of the gas?

A.  $\frac{1}{3}\frac{NV}{m}{u}^2$

B.  $\frac{1}{3}\frac{Nm}{V}{u}^2$

C.  $\frac{1}{3}\frac{N}{mV}{u}^2$

D.  $\frac{1}{3}\frac{m}{NV}{u}^2$

Calculate the maximum temperature of the gas during the cycle.

Calculate the maximum temperature of the gas during the cycle.

Calculate the maximum temperature of the gas during the cycle.

Calculate, in g, the mass of the gas.

Calculate, in g, the mass of the gas.

Calculate, in g, the mass of the gas.

Calculate, in g, the mass of the gas.

Calculate, in g, the mass of the gas.

Calculate, in g, the mass of the gas.

Discuss how the motion of the molecules of a gas gives rise to pressure in the gas.

Discuss how the motion of the molecules of a gas gives rise to pressure in the gas.

Discuss how the motion of the molecules of a gas gives rise to pressure in the gas.

The average speed of the molecules of a gas is 500 m s⁻¹. The density of the gas is 1.2 kg m⁻³. Calculate, in kPa, the pressure of the gas.

The average speed of the molecules of a gas is 500 m s⁻¹. The density of the gas is 1.2 kg m⁻³. Calculate, in kPa, the pressure of the gas.

The average speed of the molecules of a gas is 500 m s⁻¹. The density of the gas is 1.2 kg m⁻³. Calculate, in kPa, the pressure of the gas.

Calculate the average translational speed of air molecules.

Calculate the average translational speed of air molecules.

Calculate the average translational speed of air molecules.

The air is a mixture of nitrogen, oxygen and other gases. Explain why the component gases of air in the container have different average translational speeds.

The air is a mixture of nitrogen, oxygen and other gases. Explain why the component gases of air in the container have different average translational speeds.

The air is a mixture of nitrogen, oxygen and other gases. Explain why the component gases of air in the container have different average translational speeds.

The temperature of the sample is increased without a change in pressure. Outline the effect it has on the density of the gas.

The temperature of the sample is increased without a change in pressure. Outline the effect it has on the density of the gas.

The temperature of the sample is increased without a change in pressure. Outline the effect it has on the density of the gas.

the ideal gas law,

the ideal gas law,

the ideal gas law,

the kinetic energy of particles in an ideal gas.

the kinetic energy of particles in an ideal gas.

the kinetic energy of particles in an ideal gas.

A container holds a mixture of argon and helium atoms at a temperature of 37 °C.

Calculate the average translational speed of the argon atoms.

The molar mass of argon is 4.0 × 10⁻² kg mol⁻¹.

A container holds a mixture of argon and helium atoms at a temperature of 37 °C.

Calculate the average translational speed of the argon atoms.

The molar mass of argon is 4.0 × 10⁻² kg mol⁻¹.

A container holds a mixture of argon and helium atoms at a temperature of 37 °C.

Calculate the average translational speed of the argon atoms.

The molar mass of argon is 4.0 × 10⁻² kg mol⁻¹.

Calculate the pressure of the gas in the container.

Calculate the pressure of the gas in the container.

Calculate the pressure of the gas in the container.

Determine the mass of the gas in the container.

Determine the mass of the gas in the container.

Determine the mass of the gas in the container.

Calculate the average translational speed of the gas particles.

Calculate the average translational speed of the gas particles.

Calculate the average translational speed of the gas particles.

The temperature of the gas in the container is increased.

Explain, using the kinetic theory, how this change leads to a change in pressure in the container.

The temperature of the gas in the container is increased.

Explain, using the kinetic theory, how this change leads to a change in pressure in the container.

The temperature of the gas in the container is increased.

Explain, using the kinetic theory, how this change leads to a change in pressure in the container.

Three statements about Boltzmann’s constant k_B are:

I.   k_B has a unit of J K⁻¹

II.  k_B $=\frac{\text{gas constant}}{\text{Avogadro's constant}}$

III. k_B $=\frac{\text{the average kinetic energy of particles}}{\text{temperature of the gas}}$

Which statements are correct?

A.  I and II only

B.  I and III only

C.  II and III only

D.  I, II and III

Three statements about Boltzmann’s constant k_B are:

I.   k_B has a unit of J K⁻¹

II.  k_B $=\frac{\text{gas constant}}{\text{Avogadro's constant}}$

III. k_B $=\frac{\text{the average kinetic energy of particles}}{\text{temperature of the gas}}$

Which statements are correct?

A.  I and II only

B.  I and III only

C.  II and III only

D.  I, II and III

Gases in the atmosphere are compounds of ${}_6{}^{12}\text{C}$, ${}_1{}^1\text{H}$, ${}_8{}^{16}\text{O}$ and ${}_7{}^{14}\text{N}$.

Four of these gases are CO₂, N₂O, CH₄ and H₂O. A pure sample of each gas is produced. Each sample has the same mass.

Which sample contains the greatest number of molecules?

A.  N₂O

B.  H₂O

C.  CO₂

D.  CH₄

Gases in the atmosphere are compounds of ${}_6{}^{12}\text{C}$, ${}_1{}^1\text{H}$, ${}_8{}^{16}\text{O}$ and ${}_7{}^{14}\text{N}$.

Four of these gases are CO₂, N₂O, CH₄ and H₂O. A pure sample of each gas is produced. Each sample has the same mass.

Which sample contains the greatest number of molecules?

A.  N₂O

B.  H₂O

C.  CO₂

D.  CH₄

The water is heated. Explain why the quantity of air in the storage tank decreases.

The water is heated. Explain why the quantity of air in the storage tank decreases.

The water is heated. Explain why the quantity of air in the storage tank decreases.

Two containers, $\mathrm{X}$ and $\mathrm{Y}$, are filled with an ideal gas at the same pressure.

The volume of $\mathrm{X}$ is four times the volume of $\mathrm{Y}$. The temperature of $\mathrm{X}$ is 327 °C and the temperature of $\mathrm{Y}$ is 27 °C.

What is $\frac{\mathrm{amount} \mathrm{of} \mathrm{substance} \mathrm{in} \mathrm{X}}{\mathrm{amount} \mathrm{of} \mathrm{substance} \mathrm{in} \mathrm{Y}}$ ?

A.  $\frac{1}{8}$

B.  $\frac{1}{2}$

C.  $2$

D.  $8$

Two containers, $\mathrm{X}$ and $\mathrm{Y}$, are filled with an ideal gas at the same pressure.

The volume of $\mathrm{X}$ is four times the volume of $\mathrm{Y}$. The temperature of $\mathrm{X}$ is 327 °C and the temperature of $\mathrm{Y}$ is 27 °C.

What is $\frac{\mathrm{amount} \mathrm{of} \mathrm{substance} \mathrm{in} \mathrm{X}}{\mathrm{amount} \mathrm{of} \mathrm{substance} \mathrm{in} \mathrm{Y}}$ ?

A.  $\frac{1}{8}$

B.  $\frac{1}{2}$

C.  $2$

D.  $8$

Two containers, $\mathrm{X}$ and $\mathrm{Y}$, are filled with an ideal gas at the same pressure.

The volume of $\mathrm{X}$ is four times the volume of $\mathrm{Y}$. The temperature of $\mathrm{X}$ is 327 °C and the temperature of $\mathrm{Y}$ is 27 °C.

What is $\frac{\mathrm{amount} \mathrm{of} \mathrm{substance} \mathrm{in} \mathrm{X}}{\mathrm{amount} \mathrm{of} \mathrm{substance} \mathrm{in} \mathrm{Y}}$ ?

A.  $\frac{1}{8}$

B.  $\frac{1}{2}$

C.  $2$

D.  $8$

Two containers, $\mathrm{X}$ and $\mathrm{Y}$, are filled with an ideal gas at the same pressure.

The volume of $\mathrm{X}$ is four times the volume of $\mathrm{Y}$. The temperature of $\mathrm{X}$ is 327 °C and the temperature of $\mathrm{Y}$ is 27 °C.

What is $\frac{\mathrm{amount} \mathrm{of} \mathrm{substance} \mathrm{in} \mathrm{X}}{\mathrm{amount} \mathrm{of} \mathrm{substance} \mathrm{in} \mathrm{Y}}$ ?

A.  $\frac{1}{8}$

B.  $\frac{1}{2}$

C.  $2$

D.  $8$

Two containers, $\mathrm{X}$ and $\mathrm{Y}$, are filled with an ideal gas at the same pressure.

The volume of $\mathrm{X}$ is four times the volume of $\mathrm{Y}$. The temperature of $\mathrm{X}$ is 327 °C and the temperature of $\mathrm{Y}$ is 27 °C.

What is $\frac{\mathrm{amount} \mathrm{of} \mathrm{substance} \mathrm{in} \mathrm{X}}{\mathrm{amount} \mathrm{of} \mathrm{substance} \mathrm{in} \mathrm{Y}}$ ?

A.  $\frac{1}{8}$

B.  $\frac{1}{2}$

C.  $2$

D.  $8$

Two containers, $\mathrm{X}$ and $\mathrm{Y}$, are filled with an ideal gas at the same pressure.

The volume of $\mathrm{X}$ is four times the volume of $\mathrm{Y}$. The temperature of $\mathrm{X}$ is 327 °C and the temperature of $\mathrm{Y}$ is 27 °C.

What is $\frac{\mathrm{amount} \mathrm{of} \mathrm{substance} \mathrm{in} \mathrm{X}}{\mathrm{amount} \mathrm{of} \mathrm{substance} \mathrm{in} \mathrm{Y}}$ ?

A.  $\frac{1}{8}$

B.  $\frac{1}{2}$

C.  $2$

D.  $8$

Two containers, $\mathrm{X}$ and $\mathrm{Y}$, are filled with an ideal gas at the same pressure.

The volume of $\mathrm{X}$ is four times the volume of $\mathrm{Y}$. The temperature of $\mathrm{X}$ is 327 °C and the temperature of $\mathrm{Y}$ is 27 °C.

What is $\frac{\mathrm{amount} \mathrm{of} \mathrm{substance} \mathrm{in} \mathrm{X}}{\mathrm{amount} \mathrm{of} \mathrm{substance} \mathrm{in} \mathrm{Y}}$ ?

A.  $\frac{1}{8}$

B.  $\frac{1}{2}$

C.  $2$

D.  $8$

Two containers, $\mathrm{X}$ and $\mathrm{Y}$, are filled with an ideal gas at the same pressure.

The volume of $\mathrm{X}$ is four times the volume of $\mathrm{Y}$. The temperature of $\mathrm{X}$ is 327 °C and the temperature of $\mathrm{Y}$ is 27 °C.

What is $\frac{\mathrm{amount} \mathrm{of} \mathrm{substance} \mathrm{in} \mathrm{X}}{\mathrm{amount} \mathrm{of} \mathrm{substance} \mathrm{in} \mathrm{Y}}$ ?

A.  $\frac{1}{8}$

B.  $\frac{1}{2}$

C.  $2$

D.  $8$

Two containers, $\mathrm{X}$ and $\mathrm{Y}$, are filled with an ideal gas at the same pressure.

The volume of $\mathrm{X}$ is four times the volume of $\mathrm{Y}$. The temperature of $\mathrm{X}$ is 327 °C and the temperature of $\mathrm{Y}$ is 27 °C.

What is $\frac{\mathrm{amount} \mathrm{of} \mathrm{substance} \mathrm{in} \mathrm{X}}{\mathrm{amount} \mathrm{of} \mathrm{substance} \mathrm{in} \mathrm{Y}}$ ?

A.  $\frac{1}{8}$

B.  $\frac{1}{2}$

C.  $2$

D.  $8$

Two containers, $\mathrm{X}$ and $\mathrm{Y}$, are filled with an ideal gas at the same pressure.

The volume of $\mathrm{X}$ is four times the volume of $\mathrm{Y}$. The temperature of $\mathrm{X}$ is 327 °C and the temperature of $\mathrm{Y}$ is 27 °C.

What is $\frac{\mathrm{amount} \mathrm{of} \mathrm{substance} \mathrm{in} \mathrm{X}}{\mathrm{amount} \mathrm{of} \mathrm{substance} \mathrm{in} \mathrm{Y}}$ ?

A.  $\frac{1}{8}$

B.  $\frac{1}{2}$

C.  $2$

D.  $8$

The equation $\frac{pV}{T}$ = constant is applied to a real gas where p is the pressure of the gas, V is its volume and T is its temperature.

What is correct about this equation?

A. It is empirical.

B. It is theoretical.

C. It cannot be tested.

D. It cannot be disproved.

The equation $\frac{pV}{T}$ = constant is applied to a real gas where p is the pressure of the gas, V is its volume and T is its temperature.

What is correct about this equation?

A. It is empirical.

B. It is theoretical.

C. It cannot be tested.

D. It cannot be disproved.

Cylinder X has a volume $V$ and contains 3.0 mol of an ideal gas. Cylinder Y has a volume $\frac{V}{2}$ and contains 2.0 mol of the same gas.

The gases in X and Y are at the same temperature $T$. The containers are joined by a valve which is opened so that the temperatures do not change.

What is the change in pressure in X?

A. $+\frac{1}{3}\left(\frac{RT}{V}\right)$

B. $-\frac{1}{3}\left(\frac{RT}{V}\right)$

C. $+\frac{2}{3}\left(\frac{RT}{V}\right)$

D. $-\frac{2}{3}\left(\frac{RT}{V}\right)$

Cylinder X has a volume $V$ and contains 3.0 mol of an ideal gas. Cylinder Y has a volume $\frac{V}{2}$ and contains 2.0 mol of the same gas.

The gases in X and Y are at the same temperature $T$. The containers are joined by a valve which is opened so that the temperatures do not change.

What is the change in pressure in X?

A. $+\frac{1}{3}\left(\frac{RT}{V}\right)$

B. $-\frac{1}{3}\left(\frac{RT}{V}\right)$

C. $+\frac{2}{3}\left(\frac{RT}{V}\right)$

D. $-\frac{2}{3}\left(\frac{RT}{V}\right)$

A gas storage tank of fixed volume V contains N molecules of an ideal gas at temperature T. The pressure at kelvin temperature T is 20 MPa. $\frac{N}{4}$ molecules are removed and the temperature changed to 2T. What is the new pressure of the gas?

A. 10 MPa

B. 15 MPa

C. 30 MPa

D. 40 MPa

A gas storage tank of fixed volume V contains N molecules of an ideal gas at temperature T. The pressure at kelvin temperature T is 20 MPa. $\frac{N}{4}$ molecules are removed and the temperature changed to 2T. What is the new pressure of the gas?

A. 10 MPa

B. 15 MPa

C. 30 MPa

D. 40 MPa

A container holds 20 g of argon-40(${}_{18}^{40}\text{Ar}$)  and 40 g of neon-20 (${}_{10}^{20}\text{Ne}$) .

What is$\frac{\text{number of atoms of argon -40}}{\text{number of atoms of neon -20}}$ in the container?

A. 0.25

B. 0.5

C. 2

D. 4

A container holds 20 g of argon-40(${}_{18}^{40}\text{Ar}$)  and 40 g of neon-20 (${}_{10}^{20}\text{Ne}$) .

What is$\frac{\text{number of atoms of argon -40}}{\text{number of atoms of neon -20}}$ in the container?

A. 0.25

B. 0.5

C. 2

D. 4

Show that the number of helium atoms in the container is 4 × 10²⁰.

Show that the number of helium atoms in the container is 4 × 10²⁰.

Show that the number of helium atoms in the container is 4 × 10²⁰.

Calculate the ratio $\frac{\text{volume of helium atoms}}{\text{volume of helium gas}}$.

Calculate the ratio $\frac{\text{volume of helium atoms}}{\text{volume of helium gas}}$.

Calculate the ratio $\frac{\text{volume of helium atoms}}{\text{volume of helium gas}}$.

Discuss, by reference to the kinetic model of an ideal gas and the answer to (c)(i), whether the assumption that helium behaves as an ideal gas is justified.

Discuss, by reference to the kinetic model of an ideal gas and the answer to (c)(i), whether the assumption that helium behaves as an ideal gas is justified.

Discuss, by reference to the kinetic model of an ideal gas and the answer to (c)(i), whether the assumption that helium behaves as an ideal gas is justified.

The molar mass of helium is 4.0 g mol^-1. Show that the mass of a helium atom is 6.6 × 10^-27 kg.

The molar mass of helium is 4.0 g mol^-1. Show that the mass of a helium atom is 6.6 × 10^-27 kg.

The molar mass of helium is 4.0 g mol^-1. Show that the mass of a helium atom is 6.6 × 10^-27 kg.

Show that the number of helium atoms in the container is about 4 × 10²⁰.

Show that the number of helium atoms in the container is about 4 × 10²⁰.

Show that the number of helium atoms in the container is about 4 × 10²⁰.

Calculate the ratio  $\frac{\text{total volume of helium atoms}}{\text{volume of helium gas}}$.

Calculate the ratio  $\frac{\text{total volume of helium atoms}}{\text{volume of helium gas}}$.

Calculate the ratio  $\frac{\text{total volume of helium atoms}}{\text{volume of helium gas}}$.

Explain, using your answer to (d)(i) and with reference to the kinetic model, why this sample of helium can be assumed to be an ideal gas.

Explain, using your answer to (d)(i) and with reference to the kinetic model, why this sample of helium can be assumed to be an ideal gas.

Explain, using your answer to (d)(i) and with reference to the kinetic model, why this sample of helium can be assumed to be an ideal gas.

Two flasks P and Q contain an ideal gas and are connected with a tube of negligible volume compared to that of the flasks. The volume of P is twice the volume of Q.

P is held at a temperature of 200 K and Q is held at a temperature of 400 K.

What is mass of $\frac{\mathrm{mass} \mathrm{of} \mathrm{gas} \mathrm{in} \mathrm{P}}{\mathrm{mass} \mathrm{of} \mathrm{gas} \mathrm{in} \mathrm{Q}}$?

A. $\frac{1}{8}$

B. $\frac{1}{4}$

C. 4

D. 8

Two flasks P and Q contain an ideal gas and are connected with a tube of negligible volume compared to that of the flasks. The volume of P is twice the volume of Q.

P is held at a temperature of 200 K and Q is held at a temperature of 400 K.

What is mass of $\frac{\mathrm{mass} \mathrm{of} \mathrm{gas} \mathrm{in} \mathrm{P}}{\mathrm{mass} \mathrm{of} \mathrm{gas} \mathrm{in} \mathrm{Q}}$?

A. $\frac{1}{8}$

B. $\frac{1}{4}$

C. 4

D. 8

Two containers X and Y are maintained at the same temperature. X has volume $4 {\mathrm{m}}^3$ and Y has volume $6 {\mathrm{m}}^3$. They both hold an ideal gas. The pressure in X is $100 \mathrm{Pa}$ and the pressure in Y is $50 \mathrm{Pa}$. The containers are then joined by a tube of negligible volume. What is the final pressure in the containers?

A.  $70 \mathrm{Pa}$

B.  $75 \mathrm{Pa}$

C.  $80 \mathrm{Pa}$

D.  $150 \mathrm{Pa}$

Two containers X and Y are maintained at the same temperature. X has volume $4 {\mathrm{m}}^3$ and Y has volume $6 {\mathrm{m}}^3$. They both hold an ideal gas. The pressure in X is $100 \mathrm{Pa}$ and the pressure in Y is $50 \mathrm{Pa}$. The containers are then joined by a tube of negligible volume. What is the final pressure in the containers?

A.  $70 \mathrm{Pa}$

B.  $75 \mathrm{Pa}$

C.  $80 \mathrm{Pa}$

D.  $150 \mathrm{Pa}$

A substance in the gas state has a density about $1000$ times less than when it is in the liquid state. The diameter of a molecule is $d$. What is the best estimate of the average distance between molecules in the gas state?

A.  $d$

B.  $10d$

C.  $100d$

D.  $1000d$

A substance in the gas state has a density about $1000$ times less than when it is in the liquid state. The diameter of a molecule is $d$. What is the best estimate of the average distance between molecules in the gas state?

A.  $d$

B.  $10d$

C.  $100d$

D.  $1000d$

A sample of oxygen gas with a volume of $3.0 {\text{m}}^3$ is at $100 °\text{C}$. The gas is heated so that it expands at a constant pressure to a final volume of $6.0 {\text{m}}^3$. What is the final temperature of the gas?

A. $750 °\text{C}$

B. $470 °\text{C}$

C. $370 °\text{C}$

D. $200 °\text{C}$

A sample of oxygen gas with a volume of $3.0 {\text{m}}^3$ is at $100 °\text{C}$. The gas is heated so that it expands at a constant pressure to a final volume of $6.0 {\text{m}}^3$. What is the final temperature of the gas?

A. $750 °\text{C}$

B. $470 °\text{C}$

C. $370 °\text{C}$

D. $200 °\text{C}$

Two identical containers X and Y each contain an ideal gas. X has N molecules of gas at an absolute temperature of T and Y has 3N molecules of gas at an absolute temperature of $\frac{T}{2}$ What is the ratio of the pressures $\frac{P_Y}{P_X}$?

A.   $\frac{1}{6}$

B.   $\frac{2}{3}$

C.   $\frac{3}{2}$

D.   $6$

Two identical containers X and Y each contain an ideal gas. X has N molecules of gas at an absolute temperature of T and Y has 3N molecules of gas at an absolute temperature of $\frac{T}{2}$ What is the ratio of the pressures $\frac{P_Y}{P_X}$?

A.   $\frac{1}{6}$

B.   $\frac{2}{3}$

C.   $\frac{3}{2}$

D.   $6$

The molar mass of water is 18 g mol⁻¹. Estimate the average speed of the water molecules in the vapor produced. Assume the vapor behaves as an ideal gas.

The molar mass of water is 18 g mol⁻¹. Estimate the average speed of the water molecules in the vapor produced. Assume the vapor behaves as an ideal gas.

The molar mass of water is 18 g mol⁻¹. Estimate the average speed of the water molecules in the vapor produced. Assume the vapor behaves as an ideal gas.

The molar mass of an ideal gas is $M$. A fixed mass $m$ of the gas expands at a constant pressure $p$. The graph shows the variation with temperature T of the gas volume V.

What is the gradient of the graph?

A.  $\frac{Mp}{mR}$

B.  $\frac{MR}{mp}$

C.  $\frac{mp}{MR}$

D.  $\frac{mR}{Mp}$

The molar mass of an ideal gas is $M$. A fixed mass $m$ of the gas expands at a constant pressure $p$. The graph shows the variation with temperature T of the gas volume V.

What is the gradient of the graph?

A.  $\frac{Mp}{mR}$

B.  $\frac{MR}{mp}$

C.  $\frac{mp}{MR}$

D.  $\frac{mR}{Mp}$

A fixed mass of an ideal gas has a volume of $V$, a pressure of p and a temperature of $30 °\text{C}$. The gas is compressed to the volume of $\frac{V}{6}$ and its pressure increases to 12p. What is the new temperature of the gas?

A.  $15 °\text{C}$

B.  $60 °\text{C}$

C.  $333 °\text{C}$

D.  $606 °\text{C}$

A fixed mass of an ideal gas has a volume of $V$, a pressure of p and a temperature of $30 °\text{C}$. The gas is compressed to the volume of $\frac{V}{6}$ and its pressure increases to 12p. What is the new temperature of the gas?

A.  $15 °\text{C}$

B.  $60 °\text{C}$

C.  $333 °\text{C}$

D.  $606 °\text{C}$

An ideal gas is maintained at a temperature of 100 K. The variation of the pressure P and $\frac{1}{\text{volume}}$ of the gas is shown.

What is the quantity of the gas?

A.  $\frac{2\times {10}^5}{R} \text{mol}$

B.  $\frac{200}{R} \text{mol}$

C.  $\frac{80}{R} \text{mol}$

D.  $\frac{4}{5R} \text{mol}$

An ideal gas is maintained at a temperature of 100 K. The variation of the pressure P and $\frac{1}{\text{volume}}$ of the gas is shown.

What is the quantity of the gas?

A.  $\frac{2\times {10}^5}{R} \text{mol}$

B.  $\frac{200}{R} \text{mol}$

C.  $\frac{80}{R} \text{mol}$

D.  $\frac{4}{5R} \text{mol}$

A quantity of an ideal gas is at a temperature T in a cylinder with a movable piston that traps a length L of the gas. The piston is moved so that the length of the trapped gas is reduced to $\frac{5L}{6}$ and the pressure of the gas doubles.

What is the temperature of the gas at the end of the change?

A.  $\frac{5}{12}T$

B.  $\frac{3}{5}T$

C.  $\frac{5}{3}T$

D.  $\frac{12}{5}T$

A quantity of an ideal gas is at a temperature T in a cylinder with a movable piston that traps a length L of the gas. The piston is moved so that the length of the trapped gas is reduced to $\frac{5L}{6}$ and the pressure of the gas doubles.

What is the temperature of the gas at the end of the change?

A.  $\frac{5}{12}T$

B.  $\frac{3}{5}T$

C.  $\frac{5}{3}T$

D.  $\frac{12}{5}T$

Calculate the number of gas particles in the cylinder.

Calculate the number of gas particles in the cylinder.

Calculate the number of gas particles in the cylinder.

A vessel contains a mass X of helium gas and a mass 2X of oxygen gas.

Molar mass of helium = 4 g

Molar mass of oxygen = 32 g

What is the $\frac{\mathrm{number} \mathrm{of} \mathrm{helium} \mathrm{atoms}}{\mathrm{number} \mathrm{of} \mathrm{oxygen} \mathrm{molecules}}$?

A.  $\frac{1}{8}$

B.  $\frac{1}{4}$

C.  4

D.  8

A vessel contains a mass X of helium gas and a mass 2X of oxygen gas.

Molar mass of helium = 4 g

Molar mass of oxygen = 32 g

What is the $\frac{\mathrm{number} \mathrm{of} \mathrm{helium} \mathrm{atoms}}{\mathrm{number} \mathrm{of} \mathrm{oxygen} \mathrm{molecules}}$?

A.  $\frac{1}{8}$

B.  $\frac{1}{4}$

C.  4

D.  8

A vessel contains a mass X of helium gas and a mass 2X of oxygen gas.

Molar mass of helium = 4 g

Molar mass of oxygen = 32 g

What is the $\frac{\mathrm{number} \mathrm{of} \mathrm{helium} \mathrm{atoms}}{\mathrm{number} \mathrm{of} \mathrm{oxygen} \mathrm{molecules}}$?

A.  $\frac{1}{8}$

B.  $\frac{1}{4}$

C.  4

D.  8

A vessel contains a mass X of helium gas and a mass 2X of oxygen gas.

Molar mass of helium = 4 g

Molar mass of oxygen = 32 g

What is the $\frac{\mathrm{number} \mathrm{of} \mathrm{helium} \mathrm{atoms}}{\mathrm{number} \mathrm{of} \mathrm{oxygen} \mathrm{molecules}}$?

A.  $\frac{1}{8}$

B.  $\frac{1}{4}$

C.  4

D.  8

Calculate, in g, the mass of the gas.

Calculate, in g, the mass of the gas.

Calculate, in g, the mass of the gas.

Calculate, in g, the mass of the gas.

Calculate, in g, the mass of the gas.

Calculate, in g, the mass of the gas.

Determine, using the graph, whether the gas acts as an ideal gas.

Determine, using the graph, whether the gas acts as an ideal gas.

Determine, using the graph, whether the gas acts as an ideal gas.

Determine, using the graph, whether the gas acts as an ideal gas.

Determine, using the graph, whether the gas acts as an ideal gas.

Determine, using the graph, whether the gas acts as an ideal gas.