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26 Cards in this Set
- Front
- Back
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french for "sour wine" , from which the name vinegar is derived
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vinaigre
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sum of the atomic weights of all the atoms in a molecule
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molecular weight
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sum of the atomic weights of all the atoms in a formula unit of a compound
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formula weight
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idea of working with enormous quantities of tiny particles in groups called moles
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mole concept
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amount of a substance that contains as many molecules or formula units as the number of atoms in exactly 12 g of carbon 12
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mole
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number of atoms in exactly 12 g of carbon-12 ; to three significant figures 6.02 x 10 ^ 23
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Avogrado's number
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mass of one mole of a substance ;atomic weight, or formula or molecular weight, expressed in grams
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molar mass
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mass percentages of each element in a compound
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percentage composition
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parts per hudnred in terms of mass. Mass % of A = mass of A in the whole over mass of the whole x 100%
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mass percentage
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chemical formula of a substance with the smallest integer subscripts
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empirical formula
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calculation of the quantities of reactants and products involved in a chemical reaction
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stoichiometry
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reactant that is entirely consumed when a reaction goes to completion
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limiting reactant
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reactant that is not completely consumed when a reaction goes to completion
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excess reactant
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maximum amount of product that can be obtained in a reaction; calculated based on the limiting reactant
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theoretical yield
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amount of product obtained from an experiment determination
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actual yield
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actual yield of product from a reaction expressed as a percentage of the theoretical yield of product : = actual yield over theoretical yield x 100%
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percentage yield
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absolute temperature scale on which the units are given by K = C + 273.15
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Kelvin scale
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partial pressure of the molecules of a substance in the gaseous state in the presence of the liquid substance
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vapor pressure
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idea that a gas consists of molecules in constant random motion
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kinetic-molecular theory
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the volume of a gas at a given temperature varies inversely with the applied pressure
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Boyle's law
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the volume occupied by any sample of gas at a constant pressure is directly proportional to the absolute temperature
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Charle's law
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equal volumes of any two gases at the same temperature and pressure contain the same number of molecules
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Avogrado's law
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PV=nRT
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ideal gas law
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pressure of a given amount of gas at a fixed volume is proportional to the absolute temperature
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Amonton's law
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sum of the partial pressures of all the different gases in a mixture is equal to the total pressure of the mixture
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Dalton's law of partial pressures
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rate of effusion of gas molecules from a particular hole is inversely proportional to the square root of the molecular weight of the gas at constant T and P
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Graham's law of effusion
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