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Name ____________________________________________________________ Date __________________ Stoichiometry Before You Read Define the following terms. mole the SI base unit used to measure the amount of atoms, particles, ______________________________________________________________ or formula units in a substance ______________________________________________________________ molar mass mass in grams of one mole of any pure substance ______________________________________________________________ conversion factor a ratio of equivalent values used to express the same quantity in different units ______________________________________________________________ dimensional analysis a method of problem-solving that focuses on the units used to ______________________________________________________________ describe matter ______________________________________________________________ law of conservation of mass Chapter 9 states that mass is neither created nor destroyed during a ______________________________________________________________ chemical chemical reaction, but is conserved ______________________________________________________________ Balance the following equation. 3 Mg (s) 2 AlCl3 (aq) 2 Al (s) 3 MgCl2 (aq) Chapter 10 Use the periodic table in the back of your text to complete the chart. Pure Substance Carbon 12.011 Sodium 22.990 Oxygen 15.999 Sodium carbonate Chemistry: Matter and Change Molar Mass 143 105.96 Science Notebook Name ____________________________________________________________ Date __________________ Stoichiometry Section 1 Defining Stoichiometry Skim Section 1 of your text. Write three questions that come to mind from reading the headings and the illustration captions. Accept all reasonable responses. 1. ___________________________________________________________ 2. ___________________________________________________________ 3. ___________________________________________________________ Use your text to define each term. stoichiometry the study of quantitative relationships between amounts of ______________________________________________________________ reactants used and products formed by a chemical reaction ______________________________________________________________ mole ratio a ratio between the numbers of moles of any two substances in a ______________________________________________________________ balanced chemical equation ______________________________________________________________ Define the following term. derive Particle and Mole Relationships Use with pages 368–369. to obtain from a specified source ______________________________________________________________ Explain the importance of the law of conservation of mass in chemical reactions. The law of conservation of mass states that matter is neither ______________________________________________________________ created nor destroyed in a chemical reaction. Chemical bonds in ______________________________________________________________ reactants break and new chemical bonds form to produce ______________________________________________________________ products, but the amount of matter present at the end of the ______________________________________________________________ reaction is the same as it was at the beginning of the reaction. ______________________________________________________________ Chemistry: Matter and Change 144 Science Notebook Name ____________________________________________________________ Date __________________ Section 1 Defining Stoichiometry (continued) Interpreting Chemical Equations Use with Example Problem 1, page 370. Summarize Fill in the blanks to help you take notes while you read Example Problem 1. Problem representative particles, moles Interpret the equation in terms of ______________________________, observed mass Show that the law of conservation of mass is ___________. and _______. 1. Analyze the Problem C3H8(g) 5O2(g) 3CO2(g) 4H2O(g) Known: _____________________________________________ Unknown: _____________________________________________ The equation in terms of molecules The equation in terms of moles _____________________________________________ _____________________________________________ The equation in terms of mass 2. Solve for the Unknown molecules The coefficients indicate the number of _________________. moles The coefficients indicate the number of _________________. Use the space below to calculate the mass of each reactant and each product. Multiply the number of moles by the conversion factor, molar mass. moles of reactant grams of reactant = grams of reactant 1 mole of reactant moles of product grams of reactant = grams of product 1 mole of reactant Add the masses of the reactants. 44.09 g C3 H8 160.0 g O2 204.1 g reactants Add the masses of the products. 132.0 g CO2 72.08 g H2O 204.1 g products law of conservation of mass is observed. Does Determine if the _____________________________ the mass of the reactants equal the mass of the products? Yes ___________. 3. Evaluate the Answer Each product or reactant has 4 significant figures. Your answer must have 4 significant figures. Chemistry: Matter and Change 145 Science Notebook Name ____________________________________________________________ Date __________________ Section 1 Defining Stoichiometry (continued) Mole ratios Use with pages 371–372. Examine Relationships between coefficients can be used to write mole ratios conversion factors called ___________________. Example Given the equation 2KClO3(s) 2KCl(s) + 3O2(g) mole ratio with the other substances in the Each substance forms a _____________ reaction. Write the mole ratios that define the mole relationships in this equation. (Hint: Relate each reactant and each product to each of the other substances.) 2 mol KCIO3 2 mol KCl and 2 mol KCIO3 3 mol O2 3 mol O2 2 mol KCl and 2 mol KCIO3 2 mol KCIO3 3 mol O2 2 mol KCl and 3 mol O2 2 mol KCI You Try It Draw arrows with colored pencils that show the relationships of the substances in this equation. Write the mole ratios for the above equation. 1 mol C2H4 3 mol O2 3 mol O2 1 mol C2H4 2 mol CO2 3 mol O2 2 mol H2O 3 mol O2 Chemistry: Matter and Change 146 and 1 mol C2H4 and 3 mol O2 and and 2 mol CO2 2 mol CO2 2 mol CO2 1 mol C2H4 2 mol H2O 2 mol CO2 and 1 mol C2H4 and 3 mol O2 2 mol H2O 2 mol H2O and 2 mol CO2 and 2 mol H2O 2 mol H2O 1 mol C2H4 Science Notebook