Presentation on theme: "1 STOICHIOMETRY. 2 Introduction u We will look at quantitative measurements in chemical reactions. u Mass and mole relationships in chemical reactions."— Presentation transcript:
2 Introduction u We will look at quantitative measurements in chemical reactions. u Mass and mole relationships in chemical reactions u Limiting reagents in a reaction u Theoretical and percent yield u Solution concentrations and preparations
3 Quantitative measurements are those that involve actual, not just human judgement. Quantitative measurements are those that involve actual number relationships, not just human judgement. Ex cm, 5.42 moles, g, 24.1 L not just, “It was really, really a lot”
4 In a balanced chemical equation, the coefficients allow us to calculate how much of a substance is used, produced, or needed in the reaction. continued... N 2 + 3H > 2NH 3
5 N 2 (g) + 3H 2 (g) -----> 2NH 3 u From this equation we can determine that 1 mole of Nitrogen gas (28.02 g ) reacts with 3 moles of Hydrogen gas (6.06 g) to produce 2 moles of ammonia (28.02g g=34.08g of ammonia)
6 Ex. 1 How many moles of NaOH will react with 3.21 moles of sulfuric acid? Step 1. Always write the balanced chemical equation. Step 2. Write down the given numeric info. If it is not in mole units convert it to moles using the molecular mass as a conversion factor. continued....
7 continued... Step 3. Now convert from the moles of starting substance to the moles of the desired substance by using a mole to mole ratio from the chemical reaction.
8 continued... Step 4. If the problem is to find grams of the substance, convert the moles to grams using the molecular mass conversion factor. Step5. Check units and significant figures.
9 continued... Now lets work out the example problem : Step 1. H 2 SO 4 + 2NaOH -----> Na 2 SO 4 + 2HOH continued...
10 continued... Step 3 (Note that step 2 is not needed) 3.21 moles H 2 SO 4 x 2moles NaOH 1 mol H 2 SO 4 = 6.42 moles NaOH Are the significant figures correct?
11 Ex. 2 How many moles of Hydrogen are required to react with g of Nitrogen in the Haber Process to produce ammonia? Step 1. 3H 2 + N > 2NH 3 continued...
12 continued... Step g N 2 x 1mole N 2 = 3.68 moles g N 2 of N 2 continued...
13 continued... Step moles N 2 x 3 moles H 2 = 10.0 mole 1 mol N 2 H 2 Are the significant figures correct?
14 Ex. 3 How many grams of Hydrogen are required to react with g of Oxygen in the production of water? Step 1. 2H 2 + O > 2H 2 O continued...
15 continued... Step g O 2 x 1 mole O 2 = 3.12mol O g O 2 Step mol O 2 x 2mol H 2 = 6.24mol H 2 1 mol O 2.. continued...
16 continued... Step mol H 2 x 2.02 g H 2 = g H 2 1 mol H 2 Are the significant figures correct?
17 Remember.... In multiplication and division, the number of significant figures in the answer should be equal to the least number of significant figures in the problem. Coefficients in the chemical equation are exact numbers.
18 The Limiting Reagent We have already seen, from the chemical equations in the previous problems, that certain ratios of substances will react. In a chemical reaction, one of the substances may be in excess of the needed ratio (or one of them may be short of the needed ratio)
19 Notice that there is an excess of red atoms after the bonds have been made. There is a shortage of the green atoms. The green are the limiting reagent.
20 We must be able to calculate which substance is the limiting reagent because it will be the one to stop the reaction from continuing. Once we have done this, we can calculate, theoretically, the amount of product that should be produced. Limiting Reagent continued...
21 For example, if you need 4 slices of bread and 2 pieces of cheese to make 2 sandwiches and you have 4 slices of bread and 1 piece of cheese, the cheese is the limiting reagent. Your product will be only 1 sandwich. The process of making sandwiches will stop before you get to make the second sandwich. continued...
22 A chemical reaction works in a similar fashion but we must calculate the quantities in question. Ex. 4 Iron combines with Sulfur according to the following reaction: Fe (s) + S (l) -----> FeS (s) In an experiment, 7.62 g Fe are allowed to react with 8.67 g S. continued....
23 continued A. Determine which one of the reactants is the limiting reactant. b. Calculate the mass of FeS formed. A. 7.62g Fe x 1 mole Fe = mol Fe g Fe 8.67 g S x 1 mol S = mol S g S continued...
24 continued... We now know that we have mol Fe and mol S. Use the balanced chemical equation to determine how many moles of each will be needed to react with each other. continued...
25 continued mol Fe x 1 mol S = mol S 1 mol Fe mol S needed to react with the Fe mol S x 1 mol Fe = mol Fe 1 mol S mol Fe needed to react with the S. continued...
26 continued... Since we have moles of S and only need moles of it to completely react with the given amount of Fe, we clearly have an excess amount of S. Since we only have moles of Fe and we need moles of it to completely react with the given amount of S, the Fe is the reactant that will limit the reaction. It is the limiting reagent. continued...
27 We have completed part A. Now that we know which substance will limit the reaction we can determine how much product, FeS, will be produced. B. Since 1 mole of FeS is produced from 1 mole of Fe, then 0.136moles Fe x 1 mol FeS = mol 1 mol Fe FeS produced continued...
28 Now calculate the mass of FeS mol FeS x g FeS = 12.0 g 1 mol FeSFeS Since we had moles S and moles Fe, and the Fe was the limiting reagent, only moles of the S could react to produce moles of FeS. That leaves mole of S left unreacted (or 4.30 grams).
29 Yields of Reactions In the previous example we calculated the amount of FeS that, theoretically would be produced from the reaction. In the laboratory, due to experimental error, the yield of product is usually less than that which is calculated on paper. The yield that is produced in the lab is called the “Actual Yield”.
30 Percent Yield The percent yield is calculated by dividing the actual yield by the theoretical yield and then, because it is a percent, multiply by 100.
31 Ex. 5 In the previous problem the theoretical yield of FeS was calculated to be 12.0 g. In a lab experiment the actual yield was g. Calculate the % Yield g x 100 = % 12.0 g
32 Solutions u Calculating molar concentration, (Molarity) u Preparing dilutions u Stoichiometry of Solutions
33 Helpful formulas and definitions: M = Molarity = moles of solute liters of solution Solute Solute is the substance in the lesser quantity which is dissolved in the substance of greater quantity. Solvent Solvent is the substance in greater quantity. Solution Solution is the combined solute plus solvent.
34 To calculate a dilution... C c V c C d V d C c V c = C d V d CV C stands for concentration, V stands for volume cd c stands for concentrate, d stands for dilute
35 What this means is.... The concentration of the concentrated substance times the volume of the concentrated substance is equal to the concentration of the dilute substance times the volume of the dilute substance.
36 Dilution Ex. 6 Dilution How would you prepare 5.00 x 10 2 mL of 1.75 M HNO 3 from 8.6 M stock solution? C c V c = C d V d (8.6 M)(V) = (1.75 M)(5.00x10 2 mL) Solving for V = 102 mL of 8.6 M substance
37 So, to prepare the dilute solution... So, to prepare the dilute solution mL of the more concentrated 8.6 M solution is diluted with water up to 5.00 x 10 2 mL (500 mL) to produce the more dilute 1.75 M solution.
38 Ex. 7 Molarity What is the molarity of a solution that has 3.21 moles of HCl dissolved in 2.4 L of solution? Molarity = moles of solute = 3.21 moles HCl Liters of solution 2.4 L solution = 1.34 M
39 Molarity Ex. 8 Molarity How many grams of sodium sulfate (Na 2 SO 4 ) are required to prepare a 250 mL, M solution? Since molarity is in units of moles / liter we must change the mL into L : 250 mL x 1 L = L 1000mLcontinued...
40 continued L x moles Na 2 SO 4 1 liter solution = moles Na 2 SO moles Na 2 SO 4 x g Na 2 SO 4 1 mole Na 2 SO 4 = 24.3 g Na 2 SO 4
41 Ex. 9 Stoichiometry In the reaction of Zn with HCl, given 10.0 g of Zn, what volume of 2.50 M HCl (in mL) would be needed to completely react? We follow the steps of solving a stoichiometry problem but we include the molarity ratio in order to get volume.
42 continued... Step 1. Zn + 2HCl ----> ZnCl 2 + H 2 Step g Zn x 1 mol Zn = mol Zn g Zn continued....
43 continued... Step mol Zn x 2 mol HCl =0.306mol HCl 1 mol Zn Step mol HCl x 1.00 L soln. = L 2.50 mol HCl HCl soln. = 122 mL HCl soln.
44 You should be able to... 6 Do Stoichiometry calculations involving : 61. Mole - Mole relationships 62. Mass - Mole relationships 63. Mass - Mass relationships 64 Solutions 6Calculate the theoretical and % Yield 6Determine Molarity of a solution and prepare it 6Prepare a diluted solution 6Determine the limiting reagent