Boyle's law states that pressure is inversely proportional to volume at constant temperature, so if the volume is doubled, the pressure halves.

Boyle's law states that pressure is inversely proportional to volume at constant temperature, so if volume is doubled, pressure is halved.

Graham's law states that the rate of effusion is inversely proportional to the square root of the molar mass of the gas.

The ideal gas law is represented by the equation PV = nRT.

According to the kinetic molecular theory, gas particles are in constant motion.

Boyle's Law states that for a given mass of gas at constant temperature, the volume is inversely proportional to the pressure.

According to Charles's Law, the volume of a gas approaches zero at absolute zero, which is -273.15 °C.

According to Charles's Law, at constant pressure, the volume of a gas is directly proportional to its temperature.

'n' represents the number of moles of the gas in the ideal gas equation.

'a' accounts for the attractive forces between molecules, while 'b' accounts for the volume occupied by the gas molecules.

A gas deviates most from ideal behavior at low temperatures and high pressures due to increased intermolecular forces.

A liquid typically exhibits the highest density at room temperature, as it is not at the extremes of phase change.

Viscosity generally decreases with increasing temperature, so a liquid would have the highest viscosity at low temperatures.

Liquids generally exhibit the highest density at low temperatures.

In solids, particles are closely packed and have limited movement.

Plasma has the highest kinetic energy as the particles are highly energized and ionized.

Surface tension arises from cohesive forces between liquid molecules.

The boiling point of a liquid decreases with a decrease in atmospheric pressure.

The kinetic energy of particles increases as they gain energy to overcome intermolecular forces during melting.

According to Boyle's Law, if the volume is doubled at constant temperature, the pressure halves.

According to Boyle's Law, if the volume is halved, the pressure doubles at constant temperature.

According to Charles's law, the volume of a gas increases with an increase in temperature at constant pressure.

According to Boyle's Law, the volume of a gas decreases when pressure increases at constant temperature.

The boiling point is defined as the temperature at which the vapor pressure of a liquid equals the atmospheric pressure.

The critical point is where the liquid and gas phases become indistinguishable.

The critical temperature is the temperature above which a gas cannot be liquefied, regardless of the pressure applied.

The critical temperature is the temperature above which a gas cannot be liquefied.

Adding a solute to a solvent increases the boiling point of the solution, a phenomenon known as boiling point elevation.

Increasing pressure raises the boiling point of a liquid.

Generally, the density of liquids decreases with an increase in temperature.