Gas Laws and Kinetic Molecular Theory

Flashcards covering key concepts about gas behavior, including kinetic energy, pressure-volume relationships, and effects of temperature.

What factor affects the average kinetic energy of gas molecules?

The temperature of the substance.

How does temperature affect the average kinetic energy of molecules?

The higher the temperature, the higher the average kinetic energy.

What happens to the pressure of a gas when temperature increases at constant volume?

The pressure of the gas will increase as temperature increases.

Why does pressure increase as temperature increases in a gas at constant volume?

Kinetic energy of molecules increases, leading to more frequent collisions and greater force.

If gas A is at low pressure and gas B is at high pressure, which has more collisions per second?

Gas B has more collisions per second than gas A.

Describe the force that gas pressure exerts on the walls of its container.

The net force acts at right angles to the container’s surface.

What happens to the pressure of a gas if the volume is increased?

The pressure decreases.

How does increasing the volume of a gas affect the rate of collisions?

Molecules become more spread out, increasing time between collisions.

What relation exists between the product of pressure and volume for a fixed mass of gas at constant temperature?

The product of pressure and volume is constant.

What happens to internal energy when work is done on a gas?

The internal energy of the gas increases.

Why does the temperature of air inside a bike pump increase when it is pumped?

Work is done on the gas when compressed, increasing internal energy.

What happens to the force exerted on the container when gas volume increases?

The force exerted on the container decreases.

What is proportional to the average kinetic energy of gas molecules?

The temperature of the gas.

How does the rate of change of momentum relate to gas pressure?

Greater rate of change of momentum results in greater pressure.

What is the relationship between collisions and pressure in a gas?

More collisions per second lead to higher pressure.

What is the net effect of increased temperature on gas molecules?

Increased kinetic energy and larger number of molecular collisions.

How does the net force from gas pressure behave?”

It acts perpendicularly against the surface of the container.

Define the term 'constant volume' in the context of gas behavior.

A scenario where the volume of a gas does not change even as conditions change.

What is the mathematical representation of gas pressure and volume at constant temperature?

pV = constant.

What can be said about internal energy and temperature relationship in gases?

As internal energy increases, temperature also increases.

Why does lowering pressure reduce the rate of collisions in a gas?

Molecules are more spread out, increasing time between collisions.

In which scenario do molecular collisions become more frequent?

At higher pressures and temperatures.

What influences the kinetic molecular theory of gases?

Temperature and pressure conditions of the gas.

Explain how increased temperature contributes to gas pressure.

Increased kinetic energy leads to more frequent and forceful collisions.

What occurs to gas molecules during compression?

They move closer together, increasing their kinetic energy.

How does the physical state of a gas relate to pressure and temperature?

Gases expand and contract with changes in pressure and temperature.