Gas Laws Review

The concept of an ideal gas is used to explain

The behavior of a gas sample.

If the temperature is constant, what change in the volume would cause the pressure of an enclosed gas be reduced to one quarter of its original volume

The volume would have to increase by a factor of 4.

According to the kinetic theory, collisions between molecules in a sample of an ideal gas

Transfer energy between the gas particles.

What graph shows the pressure-temperature relationship expected for an ideal gas.

When temperature increases, pressure increases. When temperature decreases, pressure decreases.

A real gas behaves more like an ideal gas when the gas molecules are

far apart and have strong attractive forces between them.

At the same temperature and pressure, 1.0 liter of CO(g) and 1.0 liter of CO2(g) have

Equal volumes and the same number of molecules.

What statement describes particles of an ideal gas, based the kinetic molecular theory?

Gas particles have no attractive forces between them.

Under what conditions of temperature and pressure does oxygen gas behave at least like an ideal gas?

Low temperature and high pressure.

In a gaseous system at equilibrium with its surroundings, as molecules of A(g) collide with molecules go B(g) without reacting, the total energy of the gaseous system

Remains the same.

Why do real gases deviate from KMT?

1. They have volume. 2. They have forces of attraction.

Standard pressure is equal to

1 atm

What are two real gases that behave most ideally?

1. Hydrogen. 2. Helium.

Kinetic Molecular Theory:

1. Particles travel in a constant, random, straight-line motion. 2. Collisions between gas particles result in transfer of energy, but the next amount of energy system remains constant. 3. Volume of gas particles is insignificant compared to the size of the particles themselves. 4. No forces of attraction exists between particles. 5. Average kinetic energy of particles is proportional to kelvin temperature of the gas.

The kinetic molecular theory assumes that the particles of an ideal gas

Are in random, constant, straight-line motion.

According to the kinetic-molecular theory, particles of an ideal gas

Are separated by great distances, compared to their size.

This graph represents the pressure-volume relationship for an ideal gas at a constant temperature.

As temperature stays constant, pressure increases while volume decreases.

A sample of molecules is held at a constant pressure. Increasing the kelvin temperature of this gas sample causes the average kinetic energy of its molecules to

Increase and the volume of the gas sample to increase.

Moles formula

moles gas/total moles X Pt = Pi