Chemistry U4 Stoichiometry Study Guide and Stations Review Name: ______

Chemistry U4 Stoichiometry Study Guide and Stations Review Name: ______

ChemistryU4 Stoichiometry Study Guide and Stations ReviewName: ______

Ms. BoonPeriod: ____ Date: ______

Standard 3a: Chemical Reactions -- Station 3a: Balancing Equation Race – Balance the equations on a separate sheet of paper. (More Practice: pp. 293 #15, 16, 28)

Vocabulary:conservation of mass, reactant, product, subscript, coefficient, synthesis reaction, decomposition reaction, combustion reaction, single replacement/displacement, double replacement/displacement.

Skill: Balance Chemical Reaction Equations

  • Sample Problem: Balance the equation and state what type of reaction it represents.

__Fe (s) + __ O2 (g) → __ Fe2O3 (s)

Standard 3c:The mole and Avogadro’s Number -- Station 3c: Vocabulary Puzzle – Make a 3x3 grid out of the puzzle pieces matching the words with definitions or questions with answers. (More Practice: pp. 251 #19, pp. 252 #26, pp. 256 #3)

Vocabulary:mole, Avogadro’s number

Skill: Convert between # moles and # particles, atoms, ions, or molecules using Avogadro’s number

  • Sample Problem: How many molecules is 10 moles of sucrose?

Standard 3d: Molar mass and mole-gram conversions Station 3d: Molar Mass Puzzle – Make pairs of cards by matching questions with the proper answer. (More Practice: pp. 252 # 38(a) pp. 253 #41, 47, 58(c))

Vocabulary: molar mass, molecular weight, g/mol

Skill: Convert between # moles and # grams of a given molecule using the molar mass as conversion factor.

  • Sample Problem: What is the mass in grams of 5 moles of water?

Standard 3e: Stoichiometry Station 3e: Stoichiometry Practice -- The directions are on the back of this study guide. (More Practice: pp. 331 #32, 34, 35)

Vocabulary: stoichiometry, conversion factor, mole to mole, gram to gram, mole to gram, gram to mole, mole ratio, molar mass

Skill: Convert from grams or moles of one substance in a chemical reaction to grams or moles of another substance in a chemical reaction using molar masses and mole ratios as conversion factors.

  • Sample Problem: How much Copper is produced when 100 g aluminum react with excess copper chloride? (2 Al (s) + 3 CuCl2 (aq) → 3 Cu (s) + 2 AlCl3 (aq))

Standard 3f and IE 1c: Lab Skills No separate station – Station 3c puzzle covers some of the vocabulary. Review your pre-lab and lab materials for the rest of the information. (More Practice: Read pp. 312-316 problems pp. 314 #1-3)

Vocabulary Review activity: Fill in the blanks with the following word:coefficients, percent, limiting, product, excess, mole, theoretical, molar mass, actual, balance, human, systematic)

All stoichiometric calculations involving equations use ______ratios. When solving stoichiometric problems, you must ______the equation first. The ______in chemical reaction equations provide mole ratios that can be used as conversion factors. The conversion factor for converting between mass (g) and moles is the ______of the substance.

A(n) ______reactant is not completely used up in a chemical reaction. A(n) ______reactant is used up first and thus controls the quantity of ______that can be formed in a chemical reaction. The limiting reactant should be used to calculate the ______yield. The ______yield must be measured experimentally. The ______yield describes how close the actual yield is to the theoretical yield.

Experimental errors are part of any experiment. They are not bad, but they must be discussed because they affect the data. ______errors involve actions that affect data collection like dropping some product or not reading a scale correctly. ______errors cannot be fixed by being careful. They are inaccuracies inherent in the equipment, like a balance that only measured to the 0.1 g instead of 0.01 g.

Skills: Calculate the percent yield and identify the limiting and excess reactants based on a fact pattern.

  • Sample Problem: What is the percent yield of product when the theoretical yield was 5 grams and the actual yield was 2.5 grams?
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