Gas laws, solution concentration, and colligative properties tested on AP Chemistry. Front: the law, term, or formula. Back: definition or formula with a brief usage note.
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- Boyle's Law
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At constant temperature, pressure and volume of a gas are inversely proportional: PV = constant- Charles's Law
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At constant pressure, volume and absolute temperature of a gas are directly proportional: V/T = constant- Gay-Lussac's Law
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At constant volume, pressure and absolute temperature of a gas are directly proportional: P/T = constant- Combined Gas Law
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PV/T = constant for a fixed amount of gas, combines Boyle's and Charles's Laws- Ideal Gas Law
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PV = nRT, where P is pressure, V is volume, n is moles, R is the gas constant, T is absolute temperature- Gas constant R value
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0.0821 L·atm/(mol·K) or 8.314 J/(mol·K), depending on units- Dalton's Law of Partial Pressures
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The total pressure of a gas mixture equals the sum of the partial pressures of each individual gas: P(total) = P1 + P2 + P3...- Graham's Law of Effusion
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The rate of effusion of a gas is inversely proportional to the square root of its molar mass: rate1/rate2 = sqrt(M2/M1)- Molarity
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Moles of solute per liter of solution, M = n/V, the most common concentration unit in AP Chemistry- Molality
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Moles of solute per kilogram of solvent, m = n/kg solvent, does not change with temperature- Normality
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Equivalents of solute per liter of solution, N = eq/V, often used for acids and bases- Parts per million (ppm)
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Mass of solute per million parts of solution, ppm = (mass solute / mass solution) × 10^6, used for dilute solutions- Dilution equation
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M1V1 = M2V2, where subscripts 1 and 2 represent initial and final states- Vapor pressure lowering
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The vapor pressure of a solution is lower than pure solvent due to the presence of nonvolatile solute particles- Raoult's Law
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P(solution) = X(solvent) × P°(solvent), where X is mole fraction and P° is pure solvent vapor pressure
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