Gas Laws

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Pressure Noun

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[presh-er]

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Pressure

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The amount of force exerted by gas particles per unit area on the surface of a container.

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Example: This image shows that atmospheric pressure is higher at lower altitudes because there is a greater column of air, and therefore more weight, pressing down.

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Volume Noun

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[vol-yoom]

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Volume

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The amount of three-dimensional space a gas occupies, which is determined by the size of its container.

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Example: This image shows that as the volume of a container with gas decreases, the gas particles have less space, causing pressure to increase.

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Kinetic Energy Noun

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[ki-net-ik en-er-jee]

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Kinetic Energy

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The energy that a particle possesses due to its motion, which is directly proportional to its temperature in Kelvin.

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Example: This image of a family playing with a toy does not illustrate kinetic energy in the context of gas laws, which involves the motion of atoms and molecules.

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Kinetic Molecular Theory Noun

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[ki-net-ik mo-lek-yuh-ler thee-uh-ree]

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Kinetic Molecular Theory

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A scientific model describing a gas as numerous submicroscopic particles that are in constant, random motion.

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Example: This image shows that gas is made of tiny particles that are in constant, random motion, bouncing off each other and the container walls.

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Elastic Collision Noun

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[i-las-tik kuh-lizh-uhn]

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Elastic Collision

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A collision between particles where the total kinetic energy is conserved, meaning no energy is lost during the interaction.

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Example: Two particles (like gas molecules) collide and bounce off each other, showing how momentum is transferred in an elastic collision without losing total kinetic energy.

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Absolute Zero Noun

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[ab-suh-loot zee-roh]

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Absolute Zero

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The lowest possible theoretical temperature, 0 on the Kelvin scale, where particles of matter have minimal motion.

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Example: This diagram shows that absolute zero is the lowest possible temperature, corresponding to 0 on the Kelvin scale, -273°C, and -459°F.

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Kelvin Noun

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[kel-vin]

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Kelvin

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The SI base unit of thermodynamic temperature, using absolute zero as its null point, required for gas law calculations.

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Example: This image compares the Kelvin and Celsius temperature scales, showing key reference points like water's freezing and boiling points and the conversion formula.

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Mole Noun

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[mohl]

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Mole

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A standard scientific unit for measuring large quantities of particles, such as atoms or molecules, representing the amount of gas.

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Example: This diagram shows that one mole is a specific quantity, defined as the number of atoms in 12 grams of carbon-12 (Avogadro's number).

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Ideal Gas Constant Noun

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[ahy-deel gas kon-stuhnt]

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Ideal Gas Constant

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The proportionality constant in the ideal gas law equation, whose value depends on the units used for pressure and volume.

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Example: This image displays the Ideal Gas Law formula (PV=nRT), highlighting the variables and their units, and provides the specific numerical value for R, the Ideal Gas Constant.

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Partial Pressure Noun

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[pahr-shuhl presh-er]

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Partial Pressure

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The pressure that would be exerted by an individual gas in a mixture if it occupied the entire volume alone.

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Example: In a gas mixture, each gas exerts its own pressure. The total pressure is the sum of these individual 'partial pressures' from each gas.