1.3: Mole Ratio, Limiting & Excess Reactants, Percent Yield. Ms. Kiely Coral Gables Senior High IB Chemistry SL
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1 1.3: Mole Ratio, Limiting & Excess Reactants, Percent Yield Ms. Kiely Coral Gables Senior High IB Chemistry SL
2 Bell-Ringer #4 Which of the following are empirical formulas? I. C₆H₆ II. C₃H₈ III. N₂O₄ IV. Pb(NO₃)₂ Turn in Lab write-up
3 Bell-Ringer #4 Which of the following are empirical formulas? I. C₆H₆ II. C₃H₈ III. N₂O₄ IV. Pb(NO₃)₂ Only II and IV are empirical formulas, as their elements are in the simplest whole-number ratio. I has the empirical formula CH; III has the empirical formula NO₂
4 189 g HW Review & 20
5 14) 0.20 mol C x 8 mol H = = 0.53 mol H 3 mol C Always begin with your given value. In this problem, we were only given the value 0.20 moles of C. Within 1 mole of propane, C₃H₈, there are 3 moles of C and 8 moles of H. 15) 6.02 x 10²³ atoms of O = 1 mole O 1 mol O x 1 mol H₂SO₄ = mol H₂SO₄ 4 mol O Within 1 mole of H₂SO₄ there are 4 moles of O.
6 16) d. Molar mass of Na₂S₂O₃.5H₂O (2 x 22.99) + (2 x 32.07) + (8 x 16.00) + (10 x 1.01) = g mol ¹ 17) Use the molar mass of calcium arsenate to convert from moles to grams mol Ca₃(AsO₄)₂ x g Ca₃(AsO₄)₂ = 189 g Ca₃(AsO₄)₂ 1 mol Ca₃(AsO₄)₂ 20) g C x 6.02 x 10²³ C atoms = 18.3 x 10²³ = 1.83 x 10²⁴ C atoms g C
7 The term stoichiometry describes the relationships between reactants and products during chemical reactions. For instance, understanding how much of a reactant is needed to make a particular amount of something, or figuring out how much of your product(s) will be formed based on the amount of reactant(s) that you have. It is just like figuring out the perfect recipe! Except instead of this being a recipe for food it is a recipe for a chemical reaction.
8 How many grams of NH₃ are produced when mol of nitrogen reacts with hydrogen? You need to figure out how many grams of NH₃ you will produce, but you only know how many moles of N₂ you have. Step 1: Write out the balanced chemical equation. Step 2: Deduce the mole ratio between your substances of interest, and use this mole ratio to convert from your given substance to your substance of interest. Step 3: Convert your final answer to the desired unit if needed.
9 Step 1: Write out the balanced chemical equation. The balanced equation is necessary for solving any stoichiometry problem. The question is obviously describing a chemical reaction, which means that there must be a chemical equation. Deduce the chemical equation and make sure it is balanced. N₂(g) + 3H₂(g) 2NH₃(g) Step 2: Deduce the mole ratio between your substances of interest, and use this mole ratio to convert from your given substance to your substance of interest. Remember that the coefficients in a chemical reaction symbolize moles. Therefore you can look at the ratio between the amount of nitrogen needed and the amount of ammonia produced. Step 3: Convert your final answer to the desired unit if needed. They supplied you with moles of nitrogen, but they asked you to deduce how many grams of ammonia would be produced. Use molar mass to help you convert.
10 N₂(g) + 3H₂(g) 2NH₃(g) According to the balanced equation, 1 mole of nitrogen produces 2 moles of ammonia. This is a 1:2 mole ratio. Cross-multiply the ratio from the equation with your ratio. Cross-multiply and solve for the missing value. 1 mol N₂ x mol N₂ 2 mol NH₃ x mol NH₃ 1x = 1.20 x = 1.20 Don t forget you just solved in moles! You need grams of NH, so use NH s molar mass to convert mol NH₃ x 17.04g NH₃ 1 mol NH₃ = 20.4g NH₃
11 N₂(g) + 3H₂(g) 2NH₃(g) For some people it is easier to use dimensional analysis in stoichiometry problems. Either way, the steps are the same: mol N₂ x 2 mol NH₃ x 17.04g NH₃ 1 mol N₂ 1 mol NH₃ = 20.4g NH₃ This is the mole ratio, which is obtained from the balanced equation and helps you convert from N₂ to NH₃.
12 Imagine that you are following a recipe to make 12 cookies. It calls for you to mix 2 eggs with 4 cups of flour. You notice that you only have 1 egg, and realize that this means you will only end up using 2 out of the 4 cups of flour, and will end up producing 6 cookies. The number of eggs limited the amount of cookies produced.
13 We can refer to the egg in our situation as the Limiting Reactant and the flour as the Excess Reactant. The cookies would, of course, be the product. -Limiting reactant: the reactant in a chemical reaction that will determine how much of the product(s) will yield, i.e. the two eggs -Excess reactant: the reactant that will not be fully used since there is a limiting reactant, meaning there will be an excess of this reactant remaining, i.e. the flour
14 How many grams of NH₃ are produced when 78.90g of nitrogen reacts with 36.02g of hydrogen? You are being asked to deduce how much ammonia will be theoretically produced given the amount of reactants you have. Therefore, before you can solve for this problem, you must determine which of your reactants is limited in supply and which is in excess.
15 How many grams of NH₃ are produced when 78.90g of nitrogen reacts with 36.02g of hydrogen? Step 1: Deduce the balanced equation 1N₂(g) + 3H₂(g) 2NH₃(g) Step 2: Solve for the limiting reactant To determine the limiting reactant, make sure your reactant values are in moles. Then, divide each value by its respective coefficient g N₂ x 1 mol N₂ = mol N₂ = g N₂ g H₂ x 1 mol H₂ = mol H₂ = g H₂ 3 The lowest quotient is then the limiting reactant! Nitrogen is the limiting reactant.
16 Step 3: Solve using the mole ratio with your limiting reactant. Now that we know that nitrogen is the limiting reactant, we can solve for how much ammonia will theoretically be made given that the nitrogen will run out at some point. Hydrogen is obviously the excess reactant in this case; we will only end up using the amount of hydrogen needed to react with the limited amount of nitrogen we have g N₂ x 1 mol N₂ x 2 mol NH₃ x 17.04g NH₃ = or g NH₃ 28.02g N₂ 1 mol N₂ 1 mol NH₃ 1 mol N₂ = mol N₂ ; x = mol NH₃ ; mol NH₃ x g NH₃ = mol NH₃ x mol NH₃ 1 mol NH₃
17 Practice 1. Calculate the mass of iodine needed to prepare 28.60g of ICl: 2I₂ + KIO₃ + 6HCl 5ICl + KCl + 3H₂O 2. Nitrogen gas can be prepared from this reaction: 2NH₃ + 3 CuO ----> N₂ + 3Cu + 3H₂O 18.1g NH₃ are reacted with 90.40g CuO. Determine the theoretical yield of N₂ produced in grams.
18 Answers 1) 2)
19 Homework STUDY!!!!!! QUIZ NEXT WEEK! Friday 9/9 Worked Example questions in your book are great examples of the types of questions on the quiz :)
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