Gas Properties and Laws

These flashcards cover key concepts related to the properties of gases, gas laws, and the distinctions between ideal and real gases.

What does the Kinetic Molecular Theory (KMT) explain about gases?

It explains gas properties such as how gas particles are in constant motion, collide elastically, and have negligible volume and attraction between them.

How is absolute temperature measured in relation to kinetic energy?

Absolute temperature, measured in Kelvin, is a direct measure of the average kinetic energy of gas particles.

What are the four properties of gases?

Expansion, fluidity, low density, and compressibility.

What are the units for pressure at Standard Temperature and Pressure (STP)?

1 atm = 760 mmHg = 101.3 kPa.

What does Boyle’s Law state?

At constant temperature, the pressure of a gas is inversely proportional to its volume.

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

Gas pressure increases.

What is Dalton's Law of Partial Pressures?

The total pressure of a gas mixture is equal to the sum of the partial pressures of individual gases.

What is Graham's Law concerning gas behavior?

The rate of effusion of a gas is inversely proportional to the square root of its molar mass.

What are ideal gases and how do they differ from real gases?

Ideal gases follow gas laws perfectly under all conditions, while real gases have volume and intermolecular attractions, causing deviations from ideal behavior.

What does the Combined Gas Law state?

It combines Boyle’s, Charles’, and Gay-Lussac’s laws and describes the relationship between pressure, temperature, and volume of a gas.

How can you calculate the new pressure of a gas if its volume is decreased at a constant temperature?

Using Boyle's Law: P1V1 = P2V2.

What conditions favor ideal gas behavior?

High temperature and low pressure.

What is the formula for kinetic energy?

Kinetic energy (KE) = ½ mv², where m is mass and v is velocity.

How can you convert Celsius to Kelvin?

Add 273 to the Celsius temperature.

What happens to gas particles as the temperature increases?

They collide more frequently and with greater energy, increasing pressure if volume is constant.

What defines a real gas at typical conditions?

Real gases behave like ideal gases at high temperatures and low pressures.