In the kinetic theory model, it is assumed that there are many identical particles moving at random. State two other assumptions made in deriving the equation $pV = \frac{1}{3} Nm \langle c_{ms}^{2} \rangle$. 0 2 . 2 Explain why molecules of a gas exert a force on the walls of a container. Refer to Newton's laws of motion in your answer. 0 2 . 3 A sealed flask of volume 0.35 m³ contains an ideal gas at a pressure of 220 kPa. The mean kinetic energy of the gas molecules is 6.7 × 10⁻¹³ J. Calculate the amount of gas in the container. amount of gas = __________________________ mol 0 2 . 4 Figure 2 shows the variation of pressure with volume for a fixed mass of an ideal gas at constant absolute temperature T: Draw, on Figure 2, the graph for the same gas at temperature 2T.

A-Level AQA Physics Ideal Gases: In the kinetic theory model, it

In the kinetic theory model, it is assumed that there are many identical particles moving at random - AQA - A-Level Physics - Question 2 - 2022 - Paper 2

Question 2

In the kinetic theory model, it is assumed that there are many identical particles moving at random. State two other assumptions made in deriving the equation $pV =... show full transcript

Worked Solution & Example Answer:In the kinetic theory model, it is assumed that there are many identical particles moving at random - AQA - A-Level Physics - Question 2 - 2022 - Paper 2

Step 1

State two other assumptions made in deriving the equation $pV = \frac{1}{3} Nm \langle c_{ms}^{2} \rangle$

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Answer

The volume occupied by the gas molecules is negligible compared to the volume of the container.
Collisions between molecules are elastic, meaning kinetic energy is conserved.

Step 2

Explain why molecules of a gas exert a force on the walls of a container.

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Answer

Molecules of a gas exert a force on the walls of a container due to collisions. As the molecules move randomly and collide with the walls, they change direction and momentum. According to Newton's second law, a change in momentum results in a force being exerted on the wall of the container.

Step 3

Calculate the amount of gas in the container.

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Answer

To find the number of moles of gas, we can use the ideal gas equation:

$PV = nRT$

Given:

Pressure, $P = 220$ kPa = $220,000$ Pa
Volume, $V = 0.35 \, m^3$
R (ideal gas constant) = $8.31 \, J/(mol \, K)$ .

Rearranging for $n$ gives: $n = \frac{PV}{RT}$ Substituting the known values: $n = \frac{(220,000)(0.35)}{(8.31)(T)}$ Assuming room temperature $T = 298 \, K$ : $n = \frac{(220,000)(0.35)}{(8.31)(298)} \approx 2.69 \, mol$

Step 4

Draw, on Figure 2, the graph for the same gas at temperature 2T.

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Answer

To draw the graph for the same gas at temperature 2T, the curve on Figure 2 would shift to the right. This is because, at higher temperatures, for a fixed number of moles, the pressure for the same volume of gas increases. This will reflect a more considerable decrease in pressure with increasing volume and illustrate the characteristics of the gas at higher temperatures.

In the kinetic theory model, it is assumed that there are many identical particles moving at random - AQA - A-Level Physics - Question 2 - 2022 - Paper 2

Worked Solution & Example Answer:In the kinetic theory model, it is assumed that there are many identical particles moving at random - AQA - A-Level Physics - Question 2 - 2022 - Paper 2

State two other assumptions made in deriving the equation $pV = \frac{1}{3} Nm \langle c_{ms}^{2} \rangle$

Explain why molecules of a gas exert a force on the walls of a container.

Calculate the amount of gas in the container.

Draw, on Figure 2, the graph for the same gas at temperature 2T.

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