Introduction to Stoichiometry Worksheet with Answers, Exercises of Chemistry

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Chapter 9: Stoichiometry Stoichiometry A. Relating the mass of the _! is_Dtoarchiomatny ‘ 1. Stoichiometry follows the Law of Conservation of [Y\G‘Ss 2. The total sum of the {OSS for reactants will eepucn the total sum of the mass of the products and NOT the number of molecules. 3. Stiochiometry is dependent on balancecl equations. ot MON Swith the mass of the products in a chemical reaction B. Stiochiometric questions investigate the amount of substance needed to react with another substance, or the amount of a particular substance produced in a chemical reaction. Stoichiometric relationships can look at: 1 MO _ to_MN ole satios. a. Mole to mole ratios relate the number of moles of any substance in a balanced chemical reaction. They are based on the balanced chemical equation. b. Example: 3H, + Ny ——— » 2NH; r 3 moles of Hz requires | mole of N, to form a moles of NH3 Therefore, 6 moles of H, should equal 4 moles of NH3. This means that 17.25 moles of H, can produce ILS moles of NH3 17.5 mol H2 (2. mol NH3 ) = 11.5 mol NH; 3 mol Hy 2. Mole to “1G calculations. a. Using a balanced chemical reaction the moles of one substance is given, and another substance has an_CCG.UCU\ b. The equation MUST be bi c. Example: 3H, + Ny ————» 2NH3 amount of grams. Using the same equation, how many grams of NH3 are produced if 10.57 moles of H) are used in a reaction? 10.57 mol H (2. mol NH ) ( 17.04 g NH3 ) = 120,08 g NH; 3 mol Ha 1 mol NH3 / \ Mole to Mole ratio Mole to gram from the BALANCED conversion with the chemical equation! molar mass from the Periodic Table d. The number of moles does NOT need to be a Lohole number.