When the gas molecules in the cylinder are given energy, their average speed increases. This means they are moving faster and colliding with the walls of the cylinder more frequently and with more force.

1. Pressure: The pressure of a gas is directly related to the number and force of its collisions with the walls of its container. So, as the gas molecules move faster and collide more frequently and forcefully with the walls of the cylinder, the pressure of the gas increases.

2. Temperature: The temperature of a gas is directly related to the average kinetic energy of its molecules, which is essentially their movement. So, as the gas molecules move faster (i.e., their average speed increases), their average kinetic energy increases. This means the temperature of the gas increases.

So, in conclusion, if a sealed cylinder of gas is given energy causing the average speed of its molecules to increase, both the pressure and the temperature of the gas in the cylinder will increase.

Question

When the gas molecules in the cylinder are given energy, their average speed increases. This means they are moving faster and colliding with the walls of the cylinder more frequently and with more force.

1. Pressure: The pressure of a gas is directly related to the number and force of its collisions with the walls of its container. So, as the gas molecules move faster and collide more frequently and forcefully with the walls of the cylinder, the pressure of the gas increases.

2. Temperature: The temperature of a gas is directly related to the average kinetic energy of its molecules, which is essentially their movement. So, as the gas molecules move faster (i.e., their average speed increases), their average kinetic energy increases. This means the temperature of the gas increases.

So, in conclusion, if a sealed cylinder of gas is given energy causing the average speed of its molecules to increase, both the pressure and the temperature of the gas in the cylinder will increase.

Knowee AI · Accepted Answer

When the gas molecules in the cylinder are given energy, their average speed increases. This means they are moving faster and colliding with the walls of the cylinder more frequently and with more force.

1. Pressure: The pressure of a gas is directly related to the number and force of its collisions with the walls of its container. So, as the gas molecules move faster and collide more frequently and forcefully with the walls of the cylinder, the pressure of the gas increases.

2. Temperature: The temperature of a gas is directly related to the average kinetic energy of its molecules, which is essentially their movement. So, as the gas molecules move faster (i.e., their average speed increases), their average kinetic energy increases. This means the temperature of the gas increases.

So, in conclusion, if a sealed cylinder of gas is given energy causing the average speed of its molecules to increase, both the pressure and the temperature of the gas in the cylinder will increase.

A cylinder is filled with a gas and then sealed, so that the gas has a fixed volume. The gas molecules are given energy so that their average speed increases. What happens to the pressure and to the temperature of the gas in the cylinder?

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