Ch. 10: Chemical Quantities
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
Help!
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| (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
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| The volum occupied by 1 mole of a gas at standard temperature and pressure (STP). | Molar Volume
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| The smallest unit into which as substance can be broken down without a change in composition, usually atoms, molecules, or ions. | Representative Particle
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| A term used to refer to the mass of a mole of any substance. | Molar Mass
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| The weighted average of the masses of the isotopes of an element. | Atomic Mass
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| The number of representative particles contained in one mole of a substance; equal to 6.02 X 10 23 particles | Avogadro's Number
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| A formula with the lowest whole number ratio of elements in a compound. H2O2 is HO. | Empirical Formula
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| The percent by mass of each element in a compound. | Percent Composition
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| Three methods for measuring the amount of a substance are by ________, by ________, and by ________. | Count, Mass, Volume
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| A mole of any substance always contains ___________ representative particles. | 6.02 X 10 23
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| The atomic mass of an element expressed in grams is the mass of a _____ of the element. | Mole
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| An __________ ___________ of a compound is the simplist whole number ratio of atoms of the elements in the compound. | Empirical Formula
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| The _________ _________ is either the same as its experimentally determined empirical formula, or it is a simple whole number multiple of it. | Molecular Formula
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| Representative Particles ----> Moles | Divide number of representative particles by 6.02 X 10 23.
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| Number of Moles ----> Mass (Grams) | Multiply number of moles by molar mass.
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| Moles ----> Representative Particles | Multiply number of moles by 6.02 X 10 23.
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| Mass (Grams) ----> Moles | Divide mass (grams) by molar mass.
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| Grams/L ----> Grams/Mole | Multiply value of Grams/L by 22.4 L.
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| Moles of Gas ----> Volume of Gas | Multiply moles of gas by 22.4 L
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| Percent Mass of Element | Mass of element divided by mass of compound, times 100%.
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