Ideal Gas Law

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Ideal Gas Noun

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[eye-deel gas]

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Ideal Gas

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A hypothetical gas with molecules of negligible size and no intermolecular forces, perfectly obeying the ideal gas law.

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Example: This image contrasts an ideal gas, where particles are far apart and don't interact, with a non-ideal gas, where particles are closer and do interact.

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Pressure Noun

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[presh-er]

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Pressure

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The force exerted per unit area on a surface, typically resulting from the collisions of gas molecules.

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Example: This image shows how the pressure of the gas inside a tire affects its shape, comparing the results of too little, too much, and correct pressure.

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Mole Noun

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[mohl]

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Mole

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The SI unit for measuring large quantities of particles, where one mole contains Avogadro's number of atoms or molecules.

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Example: This diagram shows that one mole is a specific quantity, defined as the number of atoms present in exactly 12 grams of carbon-12.

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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 a particle possesses due to its motion; the average is directly proportional to the absolute temperature.

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Example: This image shows a roller coaster cart at the top of a hill where it has maximum potential energy and zero kinetic energy (it is momentarily stopped).

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Elastic Collision Noun

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[ih-las-tik kuh-lizh-un]

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Elastic Collision

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A collision between particles in which the total kinetic energy is conserved, a key assumption for ideal gases.

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Example: This diagram shows two particles before, during, and after a collision. In an elastic collision, like those between ideal gas particles, they bounce off each other.

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Avogadro's Number Noun

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[ah-vuh-gah-drohz num-ber]

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Avogadro's Number

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The specific number of particles, approximately 6.022 x 10^23, contained in one mole of any given substance.

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Example: This image displays the value of Avogadro's number, 6.02 x 10^23, and connects it to the concept of a mole, a key quantity in chemistry.

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Molar Volume Noun

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[moh-ler vol-yoom]

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Molar Volume

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The volume occupied by one mole of a substance, typically a gas, at a specific temperature and pressure.

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Example: This image shows that one mole (6.02 x 10^23 molecules) of different gases occupies the same volume (22.4 L) at the same temperature and pressure.

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Standard Temperature and Pressure (STP) Noun

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[stan-derd tem-per-uh-cher and presh-er]

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Standard Temperature and Pressure (STP)

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A standard set of conditions for measurements, defined as a temperature of 273 K and a pressure of 1 atm.

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Example: This image defines Standard Temperature and Pressure (STP) as 0°C and 1 atm, and shows that one mole of any gas occupies 22.4 liters at STP.

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Ideal Gas Constant (R) Noun

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[eye-deel gas kon-stunt]

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Ideal Gas Constant (R)

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The proportionality constant in the ideal gas law equation, whose value depends on the units used for other variables.

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Example: This image displays multiple gas laws and equations, including the Ideal Gas Law (PV=nRT), to show where the Ideal Gas Constant (R) comes from.

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Kelvin (K) Noun

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[kel-vin]

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Kelvin (K)

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The SI base unit of thermodynamic temperature; an absolute scale where 0 K represents absolute zero, required for gas laws.

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Example: This cartoon uses a pun to teach that the Kelvin temperature scale does not use the word 'degrees,' unlike Celsius or Fahrenheit.