Chemistry Laws Flashcards

Avogadro's Law

• Equal volumes of gases at the same temperature and pressure have identical particle counts.
• Applies to various particle types: atoms, ions, molecules, and electrons.

Boyle's Law

• Inversely relates gas volume and pressure at constant temperature.
• As pressure increases, volume decreases and vice versa.

Charles' Law

• Volume of a gas at constant pressure is directly proportional to its absolute temperature.
• Indicates that higher temperatures result in greater gas volumes.

Conservation of Energy

• Energy cannot be created or destroyed, only transformed.
• This principle is encapsulated in the First Law of Thermodynamics.

Conservation of Mass

• Matter maintains its mass during chemical changes, though it may rearrange.
• This law asserts that mass is conserved in ordinary chemical reactions.

Dalton's Law

• The total pressure of a gas mixture equals the sum of its individual partial pressures.
• This principle applies to any number of gases in a mixture.

Definite Composition

• Compounds consist of two or more elements combined in specific weight ratios.
• Each compound has a fixed composition, defining its chemical identity.

Dulong & Petit's Law

• Most metals need 6.2 calories to increase the temperature of 1 gram-atomic mass by 1°C.
• This property helps in understanding the thermal behavior of metallic elements.

Faraday's Law

• The amount of an element released during electrolysis correlates with the electricity passed through.
• This relationship also considers the equivalent weight of the element involved.

First Law of Thermodynamics

• Reinforces the principle of energy conservation within the universe.
• Total energy remains constant, neither created nor eliminated.

Gay-Lussac's Law

• Gas volumes involved in reactions maintain a ratio expressible in small whole numbers.
• Relevant for understanding gas reactions and stoichiometry.

Graham's Law

• Diffusion and effusion rates of gases are inversely related to the square root of their molecular masses.
• Lighter gases diffuse or effuse faster than heavier gases.

Henry's Law

• Gas solubility in liquids correlates positively with the applied pressure.
• Especially applicable for gases that are not highly soluble.

Ideal Gas Law

• Describes the physical state of an ideal gas with the equation PV = nRT.
• P stands for pressure, V for volume, n for the number of moles, R for the gas constant, and T for temperature.

Multiple Proportions

• Elements combine in ratios of small whole numbers during reactions.
• Mass relationships between different elements provide insight into their compound formation.

Periodic Law

• Elements display periodic variations in chemical properties based on atomic numbers.
• Significant in predicting and understanding elemental behavior in reactions.

Second Law of Thermodynamics

• States that entropy, a measure of disorder, tends to increase over time.
• Indicates that heat transfer does not spontaneously occur from cold to hot areas.