What force does a particle of an ideal gas experience with a pressure of 166 kPa on an area of 2.0 m2?
83 000 N
332 000 N
0.083 N
0.332 N
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Syllabus Edition
First teaching 2014
Last exams 2024
What force does a particle of an ideal gas experience with a pressure of 166 kPa on an area of 2.0 m2?
83 000 N
332 000 N
0.083 N
0.332 N
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A fixed mass of an ideal gas is trapped in a cylinder of constant volume and its temperature is varied. Which graph shows the variation of the pressure of the gas with temperature in kelvin?
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Which row gives the correct definitions for n, N and NA?
n | N | NA | |
A. | number of molecules | Avogadro's constant | Avogadro's constant |
B. | Avogadro's constant | Avogadro's constant | number of molecules |
C. | Avogadro's constant | number of moles | number of molecules |
D. | number of moles | number of molecules | Avogadro's constant |
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A sealed container contains a mixture of helium and neon gas.
The ratio of is 5.
What is the correct ratio for ?
1
5
Dependent on the concentration of each gas
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Which statement describes a correct assumption for the kinetic model of an ideal gas?
The kinetic energy of a given molecule of the gas is constant.
The forces between each gas molecule varies.
The intermolecular potential energy of the molecules of the gas varies.
The momentum of a given molecule of the gas varies upon a collision with the container.
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The volume of an ideal gas in a container is decreased at constant temperature.
Which of the following statements are correct about the molecules of the gas?
I. Their average kinetic energy increases.
II. The frequency of the collisions per unit area of the container wall increases.
III. The pressure of the gas increases.
I only
I and III only
II and III only
I and II only
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Which of the following is not an assumption of the kinetic model of ideal gases?
All particles in the gas have different speeds.
The duration of collisions between particles is long in comparison to the time between the collisions.
There are no intermolecular forces between the particles in the gas.
Collisions with the walls of the container are elastic.
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Which graph shows the correct relationship between the volume, V ,and pressure, p, of a gas kept at a constant temperature?
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Which condition allows the behaviour of a monatomic gas, such as argon, to approximate to that of an ideal gas?
Low pressure.
High temperature.
High density.
Very low temperature.
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Which of the following is not an equation used for an ideal gas?
pV = nRT
= constant
= constant
= constant
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A fixed mass of an ideal gas is at temperature T K. The pressure is quadrupled, and the volume is halved. What is the temperature after these changes?
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A fixed mass of an ideal gas undergoes an isovolumetric change. This leads to a decrease in the pressure of the gas.
Which row describes the change in internal energy of the gas and the direction of transfer of thermal energy?
|
Internal Energy |
Direction of thermal energy transfer |
A. |
greater |
to the gas |
B. |
greater |
from the gas |
C. |
less |
to the gas |
D. |
less |
from the gas |
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A fixed mass of an ideal gas is initially at an absolute temperature, T and occupies a volume, V.
The gas is adjusted so that the final pressure of the gas is twice the magnitude of the initial pressure.
Which row of the table below, A to D, gives the correct expressions for the final volume and temperature of the gas?
|
Final volume of the gas |
Final temperature of the gas |
A. |
||
B. |
||
C. |
||
D. |
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The graphs, A to D, show the variation of pV with θ for one mole of two different gases, nitrogen and chlorine, where p is the pressure of the gas, V is the volume of the gas and θ is the temperature in °C.
Which graph shows the correct variation of pV with θ for 1 mole of each gas?
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X and Y are two flasks containing an ideal gas that are connected by a tube that has negligible volume compared with the volume of each flask. The volume of X is twice the volume of Y.
The temperature of the gas in X is kept at 200 K and the temperature of the gas in Y is kept at 400 K.
If the mass of the gas in X is MX and the mass of the gas in Y is MY, what is the ratio ?
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An ideal gas of fixed mass has a pressure, p, and volume, V. The graph shows the variation of with V at a constant temperature.
Which line represents the same gas if the thermodynamic temperature and the amount of gas are doubled?
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Given the following data:
What is the pressure of oxygen in a cubic container?
1 kPa
12 kPa
110 kPa
1200 kPa
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A sealed cylinder of radius r and length L contains an ideal gas. The gas is at pressure p and temperature T. The radius of the cylinder is halved, and the temperature is altered to maintain the same pressure.
Which of these is an expression for the new temperature of the gas?
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An ideal gas of N molecules is maintained at constant volume, V. The graph shows how temperature T varies with pressure p.
What is the gradient of the graph?
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A fish swimming in a lake expels an air bubble at a depth of 30.0 m. At this depth the temperature of the water is −33 °C and the pressure is four times the pressure at the surface. The bubble rises to the surface where the temperature is 27 °C.
What is the percentage change of the volume of the air bubble as it rises to the surface from a depth of 30.0 m?
20 %
100 %
400 %
600 %
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The variation of pressure p with temperature T is shown on the graph for a fixed mass of an ideal gas at constant volume.
What is the ratio of pressure and temperature of the ideal gas?
200 Pa K−1
300 Pa K−1
400 Pa K−1
500 Pa K−1
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A mass of 5 × 10−3 kg of Hydrogen is split between two gas bottles Y and Z. Y and Z are connected by a tube that has a negligible volume compared with the volume of each bottle.
Initially the valve X is closed and gas bottle Y has a volume 4V and contains Hydrogen at a pressure p. Gas bottle Z has a volume V and contains Hydrogen at a pressure of 3p. Y and Z are initially at the same temperature.
X is now opened.
What is the new gas pressure assuming there is no change in temperature?
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A materials scientist carries out an experiment to investigate the relationship between the volume and temperature of an ideal gas. The pressure of the gas is kept constant throughout the experiment. Two of their readings are shown below.
Temperature / °C |
Volume of gas / cm3 |
0 |
55 |
100 |
76 |
What is the value for absolute zero that can be calculated from these results?
−273.15 °C
−261.9 °C
0 °C
100 °C
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An ideal gas is initially at a temperature of 127 °C. It is heated and the root mean square velocity of the gas is then tripled. Use 1 × 10−23 as the Boltzmann Constant.
|
Kinetic Energy /J |
Temperature °C |
A. |
6 × 10−21 |
3000 |
B. |
5.4 × 10−20 |
3600 |
C. |
6 × 10−21 |
3327 |
D. |
5.4 × 10−20 |
3327 |
What are the values for the temperature of the gas and the mean kinetic energy of the molecules after it has been heated?
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A single molecule of mass 5 × 10−28 kg moves with a speed of 200 m s−1 in a rigid cubical container with a side length of 0.4 m.
Assume all collisions between the molecule and the walls of the container are perfectly elastic.
What is the average pressure exerted on the wall by the molecule?
5.0 × 10−23 Pa
1.25 × 10−22 Pa
3.125 × 10−22 Pa
6.35 × 10−20 Pa
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Air consists of 0.9% argon molecules and 0.002% neon molecules. Argon has a relative molecular mass of 40 and neon a relative molecular mass of 20.
What is the ratio of the root mean square speed of argon to that of neon molecules in the air?
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In a car factory laboratory, the atmospheric pressure is 101 kPa and the temperature is 47 °C. The pressure in the car tyre under investigation is 180 kPa and the temperature 227 °C.
Assume no air is lost from the tyre.
What is the percentage increase in the root mean square speed of the air molecules due to the experiment?
10%
20%
25%
30%
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An ideal gas is stored in a sealed container of fixed volume and has molecules with a root mean square speed of c m s−1. The temperature of the gas changes resulting in a decrease in pressure by one-third of the previous value.
What is the new expression for the root mean square speed of the molecules after the temperature has changed?
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