Unit IV: Stoichiometry

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1 Unit IV: Stoichiometry D. Calculations from chemical equations 1. Mol-mol calculations 2. Mol-gram calculations 3. Gram-gram calculations E. Limiting reactant (or reagent) F. Other applications of stoichiometry G. Theoretical and percent yields IV-1

2 Stoichiometry The study of ratios in chemistry, based on the law of conservation of mass. Atoms go in as reactants, and come out as products, changed only in their arrangement. By using stoichiometry and chemical equations we can predict the quantities involved in chemical reactions. IV-2

3 Mol to mol calculations Consider the reaction: Hydrogen gas reacts with oxygen gas to form liquid water. 2 H 2(g) + O 2(g) 2 H 2 O (l) We can write stoichiometric ratios based on the balanced chemical equation. 2 mol H 2 1 mol O 2 2 mol H 2 2 mol H 2 O 1 mol O 2 1 mol O 2 2 mol H 2 2 mol H 2 O 1 mol O 2 2 mol H 2 O IV-3

4 Mol to mol problem solving How many mol of hydrogen would be necessary to react with 3.86 mol of oxygen? Step 1. Determine the units that are needed for an answer. In this case: mol of hydrogen Step 2. Identify the given information. In this case: 3.86 mol of oxygen Step 3. Referring to our balanced chemical equation, use a stoichiometric ratio that has proper units. 2 H 2(g) + O 2(g) 2 H 2 O (l) In this case: 2 mol of H 2 1 mol O 2 IV-4

5 Mol to mol problem solving How many mol of hydrogen would be necessary to react with 3.86 mol of oxygen? The final problem set up would be: 2 mol H mol O 2 x = 7.72 mol H 2 1 mol O 2 IV-5

6 Mol-mol calculations Lecture problem 4-4 (page 119) How many mol of water will be produced from combining 4.85 mol of oxygen with excess hydrogen? Follow the steps: First write the balanced chemical equation 1. Determine the units of the answer. 2. Determine what information is given. 3. Find an apply the appropriate stoichiometric ratio from the balanced chemical equation. IV-6

7 Mol to gram Calculations LP 4-5 (pg 120) A. Hydrogen combines with oxygen to produce water. How many grams of hydrogen would be necessary to combine with mol of oxygen? B. Solid potassium reacts with liquid bromine to form potassium bromide (s). How many mol of potassium bromide will form if 20.0 g of bromine react? IV-7

8 Gram to gram Calculations Consider: How many grams of carbon (s) will react with 1.25 g of iron (III) oxide (s) to form iron metal and carbon dioxide gas? 2 Fe 2 O 3(s) + 3 C (s) 4 Fe (s) + 3 CO 2(g) 1 mol Fe 2 O 3 3 mol C g C 1.25 g Fe 2 O 3 x x x = g Fe 2 O 3 2 mol Fe 2 O 3 1 mol C = g C IV-8

9 Gram to gram Calculations Lecture problem 4-6 (pg. 121) How many grams of iron (III) hydroxide will be obtained if 23.7 grams of sodium hydroxide is reacted with iron(iii) chloride? IV-9

10 IV-E Limiting Reactant Problems When conducting a chemical reaction it is very hard to combine exact stoichiometric ratios of reactants. In practical situations one reactant is usually in excess of the other. The amount of products that will form is limited by the reactant that is present in the smaller stoichiometric amount. IV-10

11 IV-E Limiting Reactant Problems We call the reactant with the smaller stoichiometric amount: The limiting reactant The reactant with the larger stoichiometric amount is called the: The excess reactant IV-11

12 Another way to think about it Consider a cucumber sandwich. (as everyone knows the standard cucumber sandwich requires 2 slices of bread, 9 slices of cucumber, 1 dollop of cream cheese) If we have 27 slices of bread, 144 cucumber slices and 19 dollops of cream cheese, how many sandwiches can we make? Which component is our limiting reactant in this case? IV-12

13 How many grams of carbon disulfide will form if grams of carbon is mixed with grams of sulfur and allowed to react? Starting with a balanced chemical equation.. C (s) + 2 S (s) CS 2(l) First: How much carbon disulfide could be made if all the carbon reacted? g CS 2 Then: How much carbon disulfide could be made if all the sulfur reacted? g CS 2 So because it would produce the least product, sulfur is our limiting reactant. IV-13

14 How many grams of silver chloride will form from reacting 2.75 g of calcium chloride with 3.21 g of silver nitrate. 1. Write a balanced chemical equation (and check to see if a reaction would indeed occur) 2. Calculate the amount of product that could be formed based on the amount of calcium chloride 3. Calculate the amount of product that could be formed based on the amount of silver nitrate 4. The limiting reactant is the one which produces the least amount of product. 5. Using the amount of product that formed work backwards to find out how much of the excess reactant was used. Then subtract this amount from your initial quantity to determine the amount left over (or that did not react) IV-14

15 One More Example Lecture problem 4-7 on page 126. If 25.0 g of Cr (s) is allowed to react with 18.5 g of oxygen gas, how many grams of Cr 2 O 3 (s) will form? How many grams of the non-limiting reactant is left unreacted? IV-15

16 IV-F Other applications of Stoichiometry Lets try the your turn problem on page 129. (we have done these before ) What is the atomic weight and identity of a metal (X) that has 4.232g combining with excess hydrochloric acid to form g of hydrogen gas and an aqueous compound with the formula XCl 3? IV-16

17 IV-G Theoretical & Percent Yield Theoretical yield Describes the amount of something it would be possible to produce. Percent yield Compares what we actually produce with what we could have produced under perfect conditions Percent yield = x 100 Actual yield Theoretical yield IV-17

18 IV-G Theoretical & Percent Yield 3.00 mol of KClO 3 is used to produce 2.25 mol of oxygen gas as in the following reaction. 2 KClO 3(s) 2KCl + 3O (s) 2(g) Determine the theoretical yield of oxygen in mol, and the percent yield of oxygen in the reaction IV-18

19 Some Extra Practice How many grams of mercury will form if g of silver is added to an excess of mercury (II) nitrate solution? Consider: 2NaHCO 3 Na 2 CO 3 + H 2 O + CO 2 How many grams of sodium bicarbonate are required to form mol of carbon dioxide? IV-19

20 Some Extra Practice Consider the following reaction: NaOH (aq) + HCl (aq) NaCl (aq) + H 2 O (l) If 22.0 g of sodium hydroxide react with 18.2 grams of hydrochloric acid, which is the limiting reactant? How much of the excess reactant is left over? IV-20

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