States of Matter and Pressure Quiz

A state where all parts are evenly spread out.

Molecules tightly packed with strong forces.

Molecules spread apart with weaker forces, always moving.

Molecules widely spread, very weak forces. Heat makes them move faster.

Attractive forces between molecules

Forces holding a molecule together.

The process of changing from one state (solid, liquid, gas) to another state.

Solids have strong attractive forces between particles, causing them to vibrate in a fixed, organized pattern.

Particles in a solid are tightly packed and have a fixed volume that maintains a rigid shape.

Liquids have a higher density than gases but a lower density than solids.

Particles in a liquid are closer together than in a gas but further apart than in a solid.

Gases are easily compressible because there is significant space between particles.

Gas particles are in constant, random motion and fill the container they are in.

Particles in any state (solid, liquid, gas) have varying levels of kinetic energy (energy of motion).

A scale used to measure temperature, freezing point of water is 0°C, and boiling point is 100°C.

A measure of how fast particles are moving.

The total energy of the particles' motion.

Gas changing to liquid; particles slow down and clump together.

The pressure exerted by the weight of the air in the atmosphere on the surface of objects.

Force applied per unit area.

Different ways to measure how much force is applied per unit of area (e.g., pounds per square inch - psi, Pascals - Pa).

Pressure acts in all directions, not just the direction of the force.

A standard unit of pressure equal to 760 mmHg (millimeters of mercury) or 14.7 psi (pounds per square inch).

The force exerted by the atmosphere per unit area.

An instrument used to measure atmospheric pressure.

An instrument that measures pressure differences between two points.

The average pressure exerted by the Earth's atmosphere at sea level.

A common unit for standard atmospheric pressure.

A unit of atmospheric pressure, based on the height of a mercury column.

A unit of atmospheric pressure (kilopascals).

A unit of atmospheric pressure, based on the height of a mercury column (in inches).

Force per unit area.

The layer of gases surrounding the Earth.

An absence of matter or gas.

Describes the inverse relationship between pressure and volume of a gas when temperature is constant.

As one variable increases, the other decreases, keeping the other factor constant.

P₁V₁ = P₂V₂ (Pressure1 x Volume1 = Pressure2 x Volume2)

Temperature must remain the same for Boyle's Law to apply.

Force exerted per unit area.

The amount of space occupied by a gas.

The amount of gas (measured in moles) is directly proportional to the volume it occupies, if temperature and pressure are kept constant.

Increasing the number of gas molecules directly increases the gas volume, and vice versa, when pressure and temperature are constant.

Temperature must remain unchanged for Avogadro's Law to hold true, meaning no heat added or removed.

Pressure must remain unchanged for Avogadro's Law to hold true, meaning no force change.

The formula that connects volume and number of moles is    V1/n1 = V2/n2

The pressure of a gas is directly proportional to its temperature (at constant volume).

The volume of a gas is directly proportional to its temperature (at constant pressure).

A measure of the average kinetic energy of particles in a substance. Higher temperature means faster particle movement.

A unit of temperature measurement; 0 Kelvin is absolute zero (no particle motion).

Temperature for gas calculations must be in Kelvin, not Celsius.

P1V1/T1 = P2V2/T2. Used to relate pressure, volume, and temperature of gases.

Standard Temperature is 273 Kelvin (or 0°C).

Standard Pressure is 1 atmosphere (atm) and often expressed in mmHg or kPa.

Variables like pressure, volume, and temperature affect the behavior of gases in calculations.

Analyzing how different types of gases behave under various conditions.

The physical dimensions of a single gas particle.

Two gas samples at different temperatures, represented with values like 596K or 298K.

The mass of one mole of a gas.

The pressure of the gases being considered as a factor in the experiment.

In the experiment, the number of particles in each gas is considered the same.

This observation considers how particle size influences pressure, volume or temperature.