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[DOC File]CHEMISTRY WORKSHEET # 2 MOLE PROBLEMS—THE MOLE …
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One mole of water contains 6.02 x 1023 molecules of water, one mole of carbon dioxide contains 6.02 x 1023 molecules of carbon dioxide, one mole of ammonia contains 6.02 x 1023 molecules of ammonia, one mole of sodium chloride contains 6.02 x 1023 “formula units” of sodium chloride, etc.
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[DOCX File]Honors Chemistry - Unit 2
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A mole is a counting unit. just like a dozen. other examples….. Avogadro’s Number. Constant. the number of particles in exactly one mole of a pure substance. 1 mol = 6.02 X10. 23. of . anything. But most often the mole is used with . atoms, ions, formula units or molecules. Examples of Conversion Factors:
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[DOC File]Mole-Particle Practice Worksheet
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1 mole of particles = 6.02 x 1023 particles (Particle is the generic word that we use in chemistry for: molecule, formula unit, ion, atom, etc.) Hints: Always begin by writing out the formula for any compound in the problem. Remember to give your answer to the correct number of significant digits. Part One: One Step Conversion. 1.
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[DOC File]Moles Class Packet Unit 2
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The coefficients in a balanced chemical equation can be used to determine mole ratios in the reaction. (3.3c) The formula mass of a substance is the sum of the atomic masses of its atoms. The molar mass (gram formula mass) of a substance equals one mole of that substance. (3.3e) The percent composition by mass of each element in a compound can ...
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[DOC File]Chemistry I-Honors
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If the compound in #2 is known to have a molecular weigh of 160.0 g/mole, what is the true, or molecular, formula? Molecular weight of the empirical formula = 80.0 g/mole. 160.0 g/mole / 80.0 g/mole = 2; then true formula = (H4N2O3) x 2 = H8N4O6-5-When a hydrate of …
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[DOC File]Moles Class Packet Unit 2
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1. The mole represents 6.02x1023 particles such as atoms and molecules of any substance. The Molar Mass (aka gram formula mass or molecular mass) is the mass of one mole of a substance. Element’s molar masses are reported on the periodic table.
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[DOC File]NOTES – MOLAR MASS AND MOLE CONVERSIONS
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Find the empirical formula of each compound below. C4H8 b. C12H24O12 c. Si3N4 d. C4Cl10. Find the molecular formula if the empirical formula is C3H8 and the molar mass is 132 g/mol. Find the molecular formula if the empirical formula is N2O5 and the molar mass is 216 g/mol. LAB: PERCENT SUGAR IN BUBBLE GUM NAME:
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[DOC File]The Mole Notes
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Molar mass (formula mass/ grams): The sum of the atomic masses of all the atoms in a molecule. The number of grams you need to make one mole of atoms of an element is equal to the atomic mass of the element. Avogadro’s number: the number of representative particles contained in one mole of a substance. 1 pair = 2. 1 dozen = 12. 1 mole = 6.02x1023
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Mole to mole formula