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Avogadro's number
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6.02 x 1023
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Molar Mass
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the mass of one mol of a substance
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Boyle's Law (Constant Temp)
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P1V1 = P2V2
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Graph Shape
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a decreasing curve
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Charle's Law (Constant Pressure)
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V1/T1 = V2/T2
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Graph Shape
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an increasing line
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Gay-Lussac's Law (Constant Volume)
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P1/T1 = P2/T2
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Graph Shape
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an increasing line
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General Law
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P1V1/T1 = P2V2/T2
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Ideal Gas Law
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PV = nRT (R = 0.082)
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Standard Conditions (STP)
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temp = 273 K / 0 C and P = 1 atm
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Avogadro's Principle
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equal volumes of gases have equal number of particles at the same temp and pressure
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Chemical Potential Energy
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the stored energy in the structure of matter
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Heat
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the energy transferred between objects (Joules)
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Calorie
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the amount of energy required to raise 1 gram of water by 1 degree C
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Heat Content (H)
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the amount of stored heat energy per mol under constant pressure
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Change in Heat Content / Enthalpy (ΔH)
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the energy absorbed or released in a reaction
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Enthalpy Formula
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ΔH = H (products) - H (reactants)
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H (products) < H (reactants)
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the reaction is exothermic, and will have a negative value
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H (products) > H (reactants)
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the reaction is endothermic, and will have a positive value
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Hess's law
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states that regardless of the multiple stages, the total enthalpy change is the sum of all the changes
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Standard heat of formation
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The change in heat content when 1 mol of compound is formed from its elements in standard conditions
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endothermic = positive = cold reactions
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exothermic = negative = warm reactions
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the heat of formation in standard conditions = 0
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Percent composition of A in AB
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( Mass of A / Mass of AB ) x 100%
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Empirical Formula
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The simplest whole number ratio of atoms (Ex: CH)
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Molecular Formula
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The actual number of atoms in a molecule (Ex: C6H6)
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N whole Number
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N = molecular formula mass / empirical formula mass
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Hydrated Salts
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salts with water molecules in it's crystals
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when hydrated salts are heated, they lose their water
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Limiting Reactant
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the substance that is used up completely
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Excess Reactant
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the substance that is not used up and remains after the reaction
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Theoretical yield
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the largest amount of product that can be produced
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Actual Yield
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the amount produced by the experiment
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Percent Yield
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= (actual yield / theoretical yield) x 100
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a gas is comprised of molecules whose average distance between each other is greater than the size of its particles
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The particles of a gas exert no attractive forces on each other or the container
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The particles are in constant random motion
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The KE of a particle depends on its mass and velocity
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Diffusion
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the movement of particles from areas of high concentration to areas of low concentration
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Graham's Law of Diffusion
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Rate1 / Rate2 = √(molar mass 2 / molar mass 1)
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Flowing
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the movement of gases through small holes
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Pressure
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the force applied perpendicularly to the surface of an object per unit area
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SI unit
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Pascal (N/m2)
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Barometer
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measures atmospheric pressure
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Manometer
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measures the pressure of a trapped gas
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Dalton's Law of partial pressure
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the total pressure of a mixture of gases is equal to the sum of the individual pressures
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