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Copyright Sautter 2003 STIOCHIOMETRY “Measuring elements” Determing the Results of A Chemical Reaction.

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Presentation on theme: "Copyright Sautter 2003 STIOCHIOMETRY “Measuring elements” Determing the Results of A Chemical Reaction."— Presentation transcript:

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2 Copyright Sautter 2003

3 STIOCHIOMETRY “Measuring elements” Determing the Results of A Chemical Reaction

4 PREDICTING HOW MUCH OF A SUBSTANCE CAN BE MADE BY A CHEMICAL REACTION BEFORE IT IS CARRIED OUT!! STEP I ALWAYS WRITE THE EQUATION USING CHEMICAL FORMULAE AND BALANCE IT. (REMEMBER TO BE SURE YOU USE THE CORRECT SUBSCRIPTS FOR THE FORMULAE AND CHANGE ONLY THE COEFFICIENTS WHEN BALANCING THE EQUATION) EXAMPLE: CALCIUM CARBONATE (LIMESTONE) WHEN HEATED GIVES CALCIUM OXIDE (LIME) AND CARBON DIOXIDE CALCIUM = Ca (+2) CARBONATE = CO 3 (-2) CALCIUM CARBONATE = CaCO 3 OXIDE = O (-2) CALCIUM OXIDE = CaO CARBON DIOXIDE = CO 2 CaCO 3(S)  CaO (s) + CO 2(g) THERE IS ONE Ca ON EACH SIDE OF THE EQUATION, ONE C ON EACH SIDE AND THREE O ON EACH SIDE. THE EQUATION IS BALANCED!

5 IN ORDER TO PREDICT THE RESULTS OF A CHEMICAL REACTION WE MUST BE GIVEN THE QUANTITIES OF MATERIALS THAT ARE TO BE USED IN THE REACTION SUPPOSE WE ARE GIVEN 200 GRAMS OF CALCIUM CARBONATE AND ASKED TO DECIDE HOW MUCH CALCIUM OXIDE AND CARBON DIOXIDE CAN BE MADE?? WE ALREADY HAVE THE BALANCED EQUATION BUT WHAT DO WE DO NEXT?? WELL, SINCE BALANCED EQUATIONS SHOW THE NUMBER OF ATOMS AND MOLECULES INVOLVED, WE MUST WORK WITH NUMBERS OF ATOMS AND MOLECULES. REMEMBER WE COUNT ATOMS AND MOLECULES WITH MOLES. (6.02 X = 1 MOLE)

6 **REMEMBER ** TO CONVERT GRAMS (MASS) TO MOLES WE DIVIDE THE WEIGHT OF ONE MOLE FROM THE PERIODIC TABLE INTO THE GIVEN NUMBER OF GRAMS FOR EXAMPLE: SINCE CaCO 3 CONTAINS 1Ca FROM THE PERIODIC TABLE WE USE 40grams x 1 1 C FROM THE PERIODIC TABLE WE USE 12 grams x1 3 O FROM THE PERIODIC TABLE WE USE 16 grams x 3 (1x 40) + (1x 12) + (3 x 16) = 100 THE MASS OF ONE MOLE OF CALCIUM CARBONATE IS 100 grams IN OUR PROBLEM WE ARE USING 200 grams of CaCO 3 DIVIDING 200grams by 100grams per mole of CaCO 3 WE FIND THAT WE HAVE EXACTLY 2 MOLES OF THE CALCIUM CARBONATE REACTANT.

7 STEP II IN SOLVING STIOCHIOMETRY PROBLEMS THEN IS TO CONVERT THE GIVEN NUMBER OF GRAMS TO MOLES..

8 CaCO 3(S)  CaO (s) + CO 2(g) THE EQUATION SAYS THAT ONE CALCIUM CARBONATE MAKES ONE CALCIUM OXIDE. HOW MANY CALCIUM OXIDES WOULD TEN CALCIUM CARBONATES MAKES? HOW ABOUT TEN? WHAT ABOUT ONE HUNDRED CALCIUM CARBONATES? WOULDN’T THEY MAKE ONE HUNDRED CALCIUM OXIDES? OF COURSE !! THEN WHAT ABOUT A MOLE OF CALCIUM CARBONATE? WOULDN’T THEY BE EXPECTED TO MAKE A MOLE OF CALCIUM OXIDE? AND OF COURSE THEN TWO MOLES WOULD MAKE TWO MOLES!

9 STEP III IS PROBABLY THE MOST DIFFICULT ONE! IT REQUIRES US TO PUT TOGETHER THE BALANCED EQUATION FROM STEP I AND THE MOLES THAT WE CALCULATED IN STEP II !! ** REMEMBER ** HERE’S OUR BALANCED EQUATION CaCO 3(S)  CaO (s) + CO 2(g) AND HERE’S THE MOLES WE CALCULATED DIVIDING 200grams by 100grams per mole of CaCO 3 WE FIND THAT WE HAVE EXACTLY 2 MOLES OF THE CALCIUM CARBONATE REACTANT

10 CaCO 3(S)  CaO (s) + CO 2(g) WHAT ABOUT THE CARBON DIOXIDE? THE BALANCED EQUATION ALSO SAYS THAT ONE CALCIUM CARBONATE MAKES ONE CARBON DIOXIDE TOO. SO USING THE SAME LOGICAL THAT WE APPLIED TO THE CALCIUM OXIDE, IT IS OBVIOUS THAT TWO MOLES OF CALCIUM CARBONATE WILL PRODUCE EXACTLY TWO MOLES OF CARBON DIOXIDE ALSO. STEP III – USING THE BALANCED EQUATION RATIOS FOUND IN STEP I AND THE MOLES DETERMINED IN STEP II, FIND THE MOLES OF EACH PRODUCT MATERIAL FORMED.

11 STEP IV – CONVERT THE MOLES FOUND IN STEP III TO GRAMS (MASS) ** REMEMBER** TO CONVERT MOLES TO GRAMS, MULTIPLY THE MASS OF ONE MOLE FROM THE PERIODIC TABLE BY THE NUMBER OF MOLES. EXAMPLE: CaO CONTAINS 1 Ca (1 X 40grams from the Periodic Table) and 1 O (1 x 16 from the Periodic Table) THE MASS OF ONE MOLE OF CaO IS (1 x 40) + (1 x 16) = 56 grams per mole TWO MOLES OF CaO ARE FORMED THEREFORE, 2 MOLES x 56 grams per mole = 112 gram of CaO ARE FORMED IN THE REACTION CO 2 CONTAINS 1 C (1 x 12grams from the Periodic Table) and 2 O (2 x 16 grams from the Periodic Table) THE MASS OF ONE MOLE OF CO 2 IS (1 x 12) + (2 x 16) = 44 grams per moles TWO MOLES OF CO 2 ARE FORMED THEREFORE, 2 MOLES x 44 grams per mole = 88 grams of CO 2 ARE FORMED IN THE REACTION

12 CaCO 3(S)  CaO (s) + CO 2(g) 200 grams 0 grams 0 grams 2 moles 0 moles 0 moles before reaction occurs 0 grams 112 grams 88 grams 0 moles 2moles 2moles after reaction occurs STARTING TOTAL MASS = = 200 GRAMS FINAL TOTAL MASS = = 200 GRAMS (CONSERVATION OF MASS) QUESTIONS ?????

13 NOW FOR A HARDER ONE! HYDROGEN GAS REACTS WITH OXYGEN GAS TO FORM WATER. HOW MUCH HYDROGEN AND OXYGEN MUST BE COMBINED TO MAKE 45 GRAMS OF WATER? STEP I – WRITE AND BALANCE THE EQUATION HYDROGEN = H 2 (DIATOMIC ELEMENT) OXYGEN = O 2 (DIATOMIC ELEMENT) WATER = H 2 O 2 H 2(g) + 1 O 2(g)  2 H 2 O (g) THERE ARE 4 ATOMS OF HYDROGEN ON EACH SIDE AND TWO ATOMS OF OXYGEN ON EACH SIDE. THE EQUATION IS BALANCED !!

14 STEP II – CONVERT THE GIVEN GRAMS TO MOLES WATER HAS A MOLAR MASS (MASS OF ONE MOLE) FROM THE PERIODIC TABLE IS 18 GRAMS. { (2 x 1) FOR HYDROGEN AND (1 x 16) FOR OXYGEN } 45 grams of water DIVIDED BY 18 grams per mole = 2.5 moles We want to make 2.5 moles of water in our reaction.

15 STEP III – USE THE BALANCED EQUATION TO FIND THE MOLES OF REACTANT OR PRODUCT REQUIRED Here’s our balanced equation from STEP I 2 H 2(g) + 1 O 2(g)  2 H 2 O (g) TWO MOLES OF WATER ARE MADE FROM TWO MOLES OF HYDROGEN. HOW MANY MOLES OF HYDROGEN WOULD BE NEEDED TO MAKE 2.5 MOLES OF WATER? (A ONE FOR ONE RATIO) HOW ABOUT 2.5 ?? NOW FOR THE OXYGEN ! IT TAKES ONLY 1 MOLE OF OXYGEN TO MAKE 2 MOLES OF WATER, HALF AS MUCH ! (A TWO FOR ONE RATIO) THEREFORE TO MAKE 2.5 MOLES OF WATER NEEDS ONLY ½ OF 2.5 MOLES OF OXYGEN! THEREFORE 1.25 MOLES OF OXYGEN IS REQUIRED.

16 STEP IV – CONVERT MOLES OF UNKNOWN TO GRAMS SINCE WE NOW KNOW THAT 2.5 MOLES OF HYDROGEN IS REQUIRED, WE CAN MULTIPLY 2.5 TIMES 2.0 GRAMS, THE MOLAR MASS OF HYDROGEN TO GET 5.0 GRAMS OF H 2(g) NEEDED! THE MOLAR MASS OF OXYGEN IS 32 GRAMS. MULTIPLYING 32 TIMES 1.25 MOLES GIVES 40 GRAMS OF OXYGEN ARE NEEDED.

17 THEN, IN ORDER TO MAKE 45.0 GRAMS OF WATER, USING HYDROGEN GAS AND OXYGEN GAS WE HAVE CALCULATED THAT: THE MOLES OF HYDROGEN NEEDED ARE 2.5 MOLES OR 5.0 GRAMS AND THE MOLES OF OXYGEN NEEDED ARE 1.25 MOLES OR 40.0 GRAMS AND ALL OF THIS HAS BEEN DETERMINED WITHOUT EVER PICKING UP A TEST TUBE BY USING STOICHIOMETRY!!!

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19 Limiting Reactant Calculations In the reactions previously discussed, an amount of only one of the reactants was given. We assumed that we could use as much of the other reactant as we needed. Unfortunately, this is not always the case. Situations where specific amounts of both of the reactants are given are called “limiting reactant” problems. The limiting reactant is the one that runs out first! In limiting reactant problems three possibilities exist. Possibility one is that the first reactant is used up first. Possibility two is that the second reactant runs out first and possibility three is that both reactants run out at the same time.

20 Containers of nuts and bolts are to be threaded together. One nut threaded on one bolt. How many combinations Can be made ? bolts nuts Only four nut – bolt combinations can be made. The bolts have run out. The bolts are the limiting factor

21 Containers of nuts and bolts are to be threaded together. Two nuts threaded on one bolt. How many combinations Can be made ? boltsnuts Only three nut – bolt combinations can be made. The nuts have run out. The nuts are the limiting factor The one with the smallest number is not always the limiting factor. It depends on the ratio of combinations!

22 Limiting Reactant Now, let’s try a limiting factor (reactant) problem using a chemical reaction! Remember, numbers of atoms and molecules are measured in moles. The balanced equation tells us the ratio of combination of the atoms and molecules that are used to make the products. In the reaction: H 2 + I 2  2 HI, one molecule of hydrogen is combined with one molecule of iodine to give two molecules of hydrogen iodide. It is also true to say that one mole of hydrogen is combined with one mole of iodine to give two moles of hydrogen iodide. All we have really done is multiply the entire equation through by 6.02 x (1 mole).

23 Limiting Reactant H 2 + I 2  2 HI Suppose that exactly one mole of H 2 and exactly one mole of I 2 are available. In this case we can make exactly two moles of HI and no H 2 or I 2 will be left. Now, suppose that we have one mole of H 2 and two moles of I 2. Once the H 2 is used up, no more I 2 can be reacted. One mole of H 2 will use exactly one mole of I 2 leaving an extra mole of I 2 unused. The limiting reactant is H 2. It ran out first. The excess reactant is I 2. We have extra I 2. Only two moles of HI can be made. Accordingly to our balanced equation, for each H 2 used, two HI are formed. Only one mole of H 2 was used so only two moles of HI are produced. The quantity of products formed is based on the limiting reactant!

24 Limiting Reactant Problem: Given the reaction: 1Ca + 1Cl 2  1CaCl 2. If we mix 120 grams of calcium and 71 grams of chlorine, which reactant is the limiting factor? How many grams of CaCl 2 can be made? Solution: Remember that balanced equations are based on moles. We must first convert the given grams to moles. Moles for Ca = 120 / 40 = 3.0, Moles for Cl 2 = 71 / (2 x 35.5) = 1.0 From the balanced equation, 1 Ca requires exactly 1 Cl 2. Since only 1.0 mole of Cl 2 is available only 1.0 mole of Ca can be consumed and 2.0 moles of Ca remain unused. Chlorine (Cl 2 ) is the limiting reactant. The amount of product that can be formed is based on the limiting reactant. The equation tells that for each Cl 2 used, one CaCl 2 is made. Since 1.0 moles Cl 2 are used, 1.0 moles of CaCl 2 are produced. Grams CaCl 2 = 1.0 moles x (40 +2(35.5)) grams per mole = 111 g

25 Limiting Reactant Problem: Given the equation: 2Na + Cl 2  2NaCl. How many grams of NaCl can be made by reacting 69 grams of Na with 5.0 moles of Cl 2 ? Solution: Again we must work in moles. Cl 2 is already moles but Na must be converted (69 / 23 = 3.0 moles of Na) From the equation, 2Na needs 1Cl 2 (half the moles of Na) so 3 Na needs 1.5 moles of Cl 2. We have 5.0 moles of Cl 2, more than enough. Therefore all of the Na is used and Na is the limiting reactant! The amount of product is based on the limiting reactant. Since 2Na make 2NaCl, 3.0 Na will make 3.0 NaCl Grams of NaCl = 3.0 moles x ( ) gram per mole of NaCl = grams of NaCl are formed.

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