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CHEMISTRY- Ch. 10

Ch. 10: Chemical Quantities

QuestionAnswer
(Standard Temperature and Pressure) The conditions under which the volume of a gas is usually measured; standard temperature is 0 degrees celsius, and standard pressure is 101.3 kPa. STP
The volum occupied by 1 mole of a gas at standard temperature and pressure (STP). Molar Volume
The smallest unit into which as substance can be broken down without a change in composition, usually atoms, molecules, or ions. Representative Particle
A term used to refer to the mass of a mole of any substance. Molar Mass
The weighted average of the masses of the isotopes of an element. Atomic Mass
The number of representative particles contained in one mole of a substance; equal to 6.02 X 10 23 particles Avogadro's Number
A formula with the lowest whole number ratio of elements in a compound. H2O2 is HO. Empirical Formula
The percent by mass of each element in a compound. Percent Composition
Three methods for measuring the amount of a substance are by ________, by ________, and by ________. Count, Mass, Volume
A mole of any substance always contains ___________ representative particles. 6.02 X 10 23
The atomic mass of an element expressed in grams is the mass of a _____ of the element. Mole
An __________ ___________ of a compound is the simplist whole number ratio of atoms of the elements in the compound. Empirical Formula
The _________ _________ is either the same as its experimentally determined empirical formula, or it is a simple whole number multiple of it. Molecular Formula
Representative Particles ----> Moles Divide number of representative particles by 6.02 X 10 23.
Number of Moles ----> Mass (Grams) Multiply number of moles by molar mass.
Moles ----> Representative Particles Multiply number of moles by 6.02 X 10 23.
Mass (Grams) ----> Moles Divide mass (grams) by molar mass.
Grams/L ----> Grams/Mole Multiply value of Grams/L by 22.4 L.
Moles of Gas ----> Volume of Gas Multiply moles of gas by 22.4 L
Percent Mass of Element Mass of element divided by mass of compound, times 100%.
Created by: m.sickles04 on 2009-01-12



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