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Stoichiometry is a process used by chemists to determine accurate chemical quantities of both products and reactants in a chemical reaction. Stoichiometry is not possible without properly written and balanced chemical equations. Balanced chemical equations give chemists a simple way of determining the amount of product that a given amount of reactants will form ___Na + ___MgCl2 ___Mg + ___NaCl - If 2 moles of Na and 1 mole of MgCl2 are reacted, ____ moles of NaCl will be produced. - To produce 1 mole of Mg you would need ____ moles of Na. Mole : Mole ratio - determined by the coefficients of a balanced chemical equation - needed to predict the chemical quantities of any reaction ___Mg + ___O2 ___MgO What is the mole : mole ratio of magnesium (Mg) and oxygen (O2) What is the mole : mole ratio of magnesium oxide (MgO) and oxygen (O2) - Stoichiometry is like cooking. To figure out the amount of ingredients you will need use your Mole Road Map _____ : _____ _____ : _____ If you need to make 10 grams of CO2 using the following reaction how many grams of baking soda NaHCO3 will you need. + NaHCO3 HCl NaCl + H2O + CO2 To answer stoichiometric problems focus on the quantity given and the quantity you are looking for! 1) Balance the following equation: C + SO2 CS2 a. How many moles of CS2 form when 6.30 moles of C reacts? b. How many moles of C are needed to react with 7.24 moles of SO2? + CO 2) Balance the following equation: Al + CuSO4 Cu + Al2(SO4)3 a. How many grams of copper are formed when 25.0 grams of Al reacts with excess CuSO4? 3) Balance the following equation: CaCO3 CaO + CO2 a. How many moles of CO2 are formed when 250 g of CaCO3 decomposes to form CaO and CO2 b. How many grams of CO2 would be produced if 2 moles of CaCO3 decomposed? 4) You need to make 550 grams of Al2O3. Al + O2 Al2O3 a. How many liters of O2 are needed? b. How many atoms of Al are needed? To calculate the percent yield, you will need to know: % Yield = Actual Yield x 100 Theoretical Yield Actual Yield = The experiment amount of product that was produced during the laboratory experiment. Theoretical Yield = The calculated amount of product determined by stoichiometry that would be the maximum that could be produced. *Both the actual yield & theoretical yield need to be in the same unit and be the same chemical in order to compare them to determine a percent yield. 1) What is the percentage yield if 5.50 grams of hydrogen gas reacts with nitrogen gas to form 20.4 grams of ammonia (nitrogen trihydride)? 2) What is the percent yield when 2.37 grams of silver nitrate reacts with sodium hydroxide to produce water, sodium nitrate and 1.55 grams of silver oxide? *Limiting Reactant: the chemical substance that ‘runs’ out first in a chemical reaction. This is the chemical that determines how much of the product(s) are made. *The true amount of excess reactant is also determined by the limiting reactant. *Excess reactants: chemical substances that you have more than enough needed for the reaction. For example, let’s make some tricycles. We will need the following per tricycle: 1 handle bar (Hb), 1 seat (S), 3 wheels (W), 1 frame (F), 2 pedals (P) 1 Hb + 1 S + 3 W + 1 F + 2 P —> 1 HbSW3FP2 Now, if you had in your possession 30 of each item, answer the following questions. 1) How many tricycles get built? 2) How many handlebars are used? 3) How many seats are used? 4) How many wheels are used? 5) How many frames are used? 6) How many pedals are used? 7) What item is the limiting factor? Pb(NO3)2 + KI PbI2 + KNO3 1) Which substance is the limiting factor when 2.96 grams of lead (II) nitrate reacts with 3.22 grams of potassium iodide? 2) How many grams of the excess reactant will be used during this experiment? 3) When the reaction is complete, how many grams of lead (II) iodide will be created?