1. Calculating Yield L.O: To be able to calculate yield for chemical reactions

2. What does yield mean?

3. The amount of product made is called the yield. In a chemical reaction no atoms are lost or gained but sometimes the yield is not what you would expect. Theoretical yield: maximum products that are made if reactants react. Actual yield: the amount of product which actually forms

4. Can you predict exactly the mass of a yield? Sodium hydroxide + hydrochloric acid  sodium chloride + hydrogen If 10g of NaOH was used how much salt would be made? What if a company wants to make 100g sodium chloride, how much NaOH should they use?

5. Precipitation is the formation of an insoluble solid when two solutions are mixed - e.g. barium sulphate is produced by precipitation from barium nitrate and sodium sulphate solutions Write a word equation for this reaction Sodium Sulphate +Barium Nitrate  Sodium Nitrate +Barium Sulphate Na 2 SO 4 + Ba(NO 3 ) 2 → 2NaNO 3 + BaSO 4

6. 1.50cm 3 water into a 100cm 3 beaker 2.Weigh 2.6g barium nitrate 3.Combine the two and stir (until all barium nitrate is dissolved) 4.Pour this into the 250cm 3 beaker 5.Measure out 75cm 3 sodium sulphate into a 100cm 3 beaker 6.Add the two solutions together 7.Stir well (notice the white precipitate) 8.Filter the mixture using a funnel and filter paper - wash the residue with a little water 9.Can you calculate the theoretical yield of barium sulfate? Then next lesson we can compare this to the actual yield produced Barium Sulphate precipitation

7. Calculating the theoretical yield Step 1: Calculate the formula mass of the reactants Here are the mass numbers you will need: Barium = 137 Nitrogen = 14 Oxygen = 16 What is the formula mass of barium nitrate Ba(NO 3 ) 2 ? Barium = 137 x 1 = 137 Nitrogen = 14 x 2 = 28 Oxygen = (16 x 3) x 2 = 96 Total = 261

8. Step 2: Calculate the relative formula mass of barium sulphate (the product formed):BaSO 4 Barium = 137 Sulphur = 32 Oxygen = 16 And the relative formula mass is: - Barium = 137 x 1 = 137 Sulphur = 32 x 1 = 32 Oxygen = 16 x 4 = 64 Total = 233

9. Na 2 SO 4 + Ba(NO 3 ) 2 → 2NaNO 3 + BaSO 4 + 261g → + 233g This means that 261g of barium nitrate will produce a theoretical 100% yield 233g of barium sulphate. Step 3: (Scaling up or down the reaction) Now work out what the mass is of the product made from 1g of the reactant. Then multiply this by the mass of the reactant that was used So 1g of Ba(NO 3 ) 2 makes 233/261 = 0.9g of BaSO 4 2.6g of Ba(NO 3 ) 2 makes 0.9 x 2.6= 2.3g of BaSO 4

10. Calculating expected yield 1. In the following reaction if N 2 (g) is present in excess and 12 g of H 2 (g) reacts, what is the theoretical yield of NH 3 (g)? 3 H 2 (g) + N 2 (g)  2 NH 3 (g) 2.If 11.5g of sodium is reacted with chlorine what is the theoretical yield of sodium chloride 2Na(s) + Cl 2 (g)  2NaCl(s)

11. Some more practice – Calculating Mass in reactions

12. Calculating the mass of a product E.g. what mass of magnesium oxide is produced when 60g of magnesium is burned in air? Step 1: READ the equation: 2Mg + O 2 2MgO IGNORE the oxygen in step 2 – the question doesn’t ask for it Step 3: LEARN and APPLY the following 3 points: 1)48g of Mg makes 80g of MgO 2)1g of Mg makes 80/48 = 1.66g of MgO 3)60g of Mg makes 1.66 x 60 = 100g of MgO Step 2: WORK OUT the relative formula masses (M r ): 2Mg = 2 x 24 = 48 2MgO = 2 x (24+16) = 80 Work our what mass 1g makes then work out what mass 60g of mg makes

13. (Another method)Calculating the mass of a product E.g. what mass of magnesium oxide is produced when 60g of magnesium is burned in air? Step 1: READ the equation: 2Mg + O 2 2MgO IGNORE the oxygen in step 2 – the question doesn’t ask for it Step 3: work out how many moles reacted: 1)Moles = mass ÷ formula mass. 60g / 48g = 1.25 moles 2)Moles X formula mass of product = 1.25 X 80 = 100g 3)60g of Mg makes 100g of MgO Step 2: WORK OUT the relative formula masses (M r ): Mg = 24 2MgO = 2 x (24+16) = 80 Work out the mass of 2.5 moles of the product (same number of moles as the reactants)

14. 15/10/2015 Work out M r : 2H 2 O = 2 x ((2x1)+16) = 36 2H 2 = 2x2 = 4 1.36g of water produces 4g of hydrogen 2.So 1g of water produces 4/36 = 0.11g of hydrogen 3.6g of water will produce (4/36) x 6 = 0.66g of hydrogen M r : 2Ca = 2x40 = 80 2CaO = 2 x (40+16) = 112 80g produces 112g so 10g produces (112/80) x 10 = 14g of CaO M r : 2Al 2 O 3 = 2x((2x27)+(3x16)) = 204 4Al = 4x27 = 108 204g produces 108g so 100g produces (108/204) x 100 = 52.9g of Al 2 O 3 1)When water is electrolysed it breaks down into hydrogen and oxygen: 2H 2 O 2H 2 + O 2 What mass of hydrogen is produced by the electrolysis of 6g of water? 3) What mass of aluminium is produced from 100g of aluminium oxide? 2Al 2 O 3 4Al + 3O 2 2) What mass of calcium oxide is produced when 10g of calcium burns? 2Ca + O 2 2CaO

15. A high yield is important in business. Can you list any ways that business could ensure a high yield? e.g. when making nylon, plastic, perfume or margarine Give it enough time to finish Try not to loose any reactants Ensure the reactants are pure Makesure the conditions are best e.g. temperature

17. 15/10/2015 Conclusion – why isn’t it possible to collect the theorectical yield? 1)The reaction may not have completely _______ 2)The reaction may have been _______ 3)Some of the product may have been ____ 4)Some of the reactants may have produced other _______ The amount of product that is made is called the “____”. This number can be compared to the maximum theoretical amount as a percentage, called the “percentage yield”. Words – lost, yield, finished, reversible, products