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Ch. 9 Handout Learning objectives: 1. Be able to translate an equation into English. (9.1) 2. Use a mole-mole factor from a balanced chemical equation to calculate the number of moles of another substance in the reaction. (9.2) 3. Given the mass in grams of a substance in a reaction, calculate the mass in grams of another substance in the reaction. (9.3) 4. Be able to define limiting reactant. (9.4) 5. Given the actual quantity of product, determine the percent yield of a reaction. (9.5) 6. Given the heat of reaction (enthalpy change), calculate the loss or gain of heat for an exothermic or endothermic reaction. (9.6) Mole-Mole Factors The chemical equation gives us information that allows us to compare moles of a substance to moles of another substance. Question: In the chemical reaction of iron and sulfur, how many moles of sulfur are needed to react with 1.42 mol of iron? 2 Fe(s) + 3 S(s) Fe2S3(s) Question: How many moles of CO2 can be produced when 2.25 mol of C3Hs reacts? C3Hs(g) + 5 O2(g) 3 CO2(g) + 4 H20(g) Mass Calculations and Limiting Reagent Substance A Substance B ; Molar mass y : Molemole ; Molar mass : e 8 aS Ss S grams of A A moles of A factor BA moles of B B grams of B Question: How many grams of COz are produced when 54.6 g of C2H2 is burned? 2 CoH2 (g) + 5 O2(g) 4 CO2(g) + 2 H20(g) Question: How many grams of O2 are required to react with 22.5 g of C7Hie? CrHi6(/) + 11 O2(g) 7 CO2(g) + 8 H20(g)