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4.7 × 1023 molecules of neon gas is trapped in a cylinder.
(b)
Calculate the number of moles of neon gas in the cylinder.
[2]
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The molar mass of neon gas is 20 g mol–1 .
(c)
Calculate the mass of the neon gas in the cylinder.
[4]
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The cylinder containing the neon gas has a volume 5.2 m3 and pressure of 600 Pa.
(d)
Calculate the temperature of the gas.
[3]
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(a)
State what is meant by an ideal gas.
[1]
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(b)
State the conditions for a real gas to approximate to an ideal gas.
[3]
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(c)
Describe how the ideal gas constant, R, is defined.
[2]
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The graphs shows how pressure, p , varies with absolute temperature, T, for a fixed mass of an ideal gas.
(d)
Outline the changes, or otherwise, to the volume and density of the ideal gas as the absolute temperature increases.
[2]
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(a)
State three assumptions of the kinetic model of an ideal gas.
[3]
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A tank of volume 21 m3 contains 7.0 moles of an ideal monatomic gas. The temperature of the gas is 28 °C.
(b)
Calculate the average kinetic energy of the particles in the gas.
[3]
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The following paragraph explains, with reference to the kinetic model of an ideal gas, how an increase in temperature of the gas leads to an increase in pressure.
A ________ temperature implies ________ average speed and therefore higher ________. This increases the ________ transferred to the walls from ________ frequent collisions. This increased ________ per collision leads to an increased ________.
(c)
Complete the sentences using keywords from the box below.
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(d)
Calculate the pressure of the gas described in part (b).
[3]
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(a)
Sketch on both axes the change in pressure and volume for an ideal gas at constant temperature.
[2]
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(b)
Sketch the graphs in part (a) at a higher temperature.
[2]
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For an ideal gas at constant volume, the pressure, p, and temperature, T, are directly proportional:
(c)
State the equation for an initial pressure p 1 at temperature T 1 and final pressure p 2 and temperature T 2 .
[1]
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The final pressure of an ideal gas is 500 Pa and its temperature rises from 410 K to 495 K.
(d)
Calculate the initial pressure of the gas.
[3]
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When there are a large number of particles in a container, their collisions with the walls of the container give rise to gas pressure.
An ideal gas with a pressure of 166 kPa collides with the walls of its container with a force of 740 N.
(b)
Calculate the area that each particle collides on.
[4]
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An ideal gas is one that obeys the relationship
(c)
If the volume an ideal gas increases, explain how this affects the:
(i)
Pressure, if the temperature remains constant.
[1]
(ii) Temperature, if the pressure remains constant.
[1]
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The ideal gas equation can be rearranged to give
constant
This relationship only holds true under a certain condition.
(d)
State the condition required for the equation to apply to an ideal gas.
[1]
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