Avogadro’s Law

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Avogadro's Law Noun

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[ah-vuh-gah-drohz law]

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Avogadro's Law

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The principle that equal volumes of all gases at the same temperature and pressure contain an equal number of molecules.

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Example: This image shows that as the amount of gas (moles) in a balloon increases, its volume (size) also increases, demonstrating Avogadro's Law.

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Mole Noun

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[mohl]

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Mole

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A standard scientific unit, represented by 'n', for measuring the amount of a substance based on a specific number of particles.

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Example: This image shows that one mole of any element, like Carbon or Copper, always contains the same number of atoms (6.02 x 10^23).

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Molecule Noun

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[mol-uh-kyool]

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Molecule

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The smallest particle of a chemical element or compound that retains the chemical properties of that substance.

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Example: This image shows an oxygen molecule, represented by its chemical symbol O₂. A molecule is the smallest particle of a substance, like the oxygen gas we breathe.

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Avogadro's Principle Noun

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[ah-vuh-gah-drohz prin-suh-puhl]

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Avogadro's Principle

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The principle stating that one mole of any gas occupies a volume of 22.4 Liters at Standard Temperature and Pressure.

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Example: This image shows that equal volumes of different gases (like oxygen and hydrogen) at the same temperature and pressure contain the same number of particles.

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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 set of standardized conditions, 0°C and 1 atm pressure, used for experimental measurements to allow for data comparison.

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Example: Standard Temperature and Pressure (STP) are defined conditions (0°C and 1 atm) where one mole of any ideal gas occupies a volume of 22.4 liters.

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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 at a given temperature and pressure, which is 22.4 L for ideal gases at STP.

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Example: This image shows that one mole of any gas, like hydrogen or oxygen, occupies the same amount of space (volume), which is 22.4 liters.

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Stoichiometry Noun

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[stoy-kee-om-i-tree]

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Stoichiometry

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The calculation of the relative quantities of reactants and products involved in chemical reactions based on balanced equations.

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Example: This image shows a balanced chemical equation, where two molecules of hydrogen (H₂) and one molecule of oxygen (O₂) combine to form two molecules of water (H₂O).

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Molar Mass Noun

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[moh-ler mas]

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Molar Mass

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The mass of one mole of a given chemical element or compound, typically expressed in units of grams per mole (g/mol).

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Example: To find the molar mass of a compound like CO2, you add the atomic masses of each atom: one carbon (12.01) and two oxygens (16.00 each).

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Gas Stoichiometry Noun

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[gas stoy-kee-om-i-tree]

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Gas Stoichiometry

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The study of quantitative relationships between reactants and products in chemical reactions that involve gases, using moles, mass, and volume.

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Example: This diagram shows how molecules in gases rearrange during a reaction. The number of molecules (1 methane, 2 oxygen) shows the ratio needed for the reaction.

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Ideal Gas Noun

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[ahy-deel gas]

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Ideal Gas

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A hypothetical gas whose molecules have no volume or intermolecular interactions, perfectly obeying all gas laws under all conditions.

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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 interact.