Moles CHEM 110
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This 2 page Bundle was uploaded by Kylie Senn on Thursday March 3, 2016. The Bundle belongs to CHEM 110 at California Polytechnic State University San Luis Obispo taught by Professor lehr in Spring 2016. Since its upload, it has received 17 views. For similar materials see Chemical Principles I in Science at California Polytechnic State University San Luis Obispo.
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Date Created: 03/03/16
Moles -After midterm Thursday, February 1812:06 PM Collection terms 1 trio= 3 singers 1 six-pack= 6 cans cola drink 1 dozen donuts= 12 donuts • Use collection terms to make life easier Moles of particles 6.02 x 10^23 particles* (Avogadro's number) 1 mole C = 6.02 x10^23 C atoms 1 mole H2O= 6.02 x10^23 H2O molecules Avogadro's # 6.02 x 10^23 particles (ions, atoms)/ 1 mole Works with direction, just make sure units cancel. Stoichiometry -the quantitative relationship between reactants and products in a chemical reactions Molar Ratios Show the mole-to-mole between two of the substances in a balanced equation Use the coefficients of 2 substances in the equation *do not change the numbers in the balanced reaction! Chemical Calculations 4Fe + 3O2-> 2Fe2O3 Molar Mass # of grams in 1 mole of a substance Equal to the numerical value of the atomic mass AKA atomic mass= 1 mole 1 mole of carbon atoms = 12.0g 1 mole of Mg atoms= 24.3g 1 mole of Cu atoms= 63.5g Molar Mass of Compounds -the mass of one mole of the compound -calculate by adding the masses of all atoms in the compound What is the mass of 3.5 mol H2O Chem Study Guide Page 1 How many molecules of CH4 are contained in 14.2g CH4? Chem Study Guide Page 2
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