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1 0 1 Limestone is mainly calcium carbonate. The formula of calcium carbonate is ao 3. omplete Table 1 to show the number of atoms in limestone. Table 1 Element Symbol Number of atoms... a... carbon oxygen The mass number of an atom is the sum of two other sub-atomic particles. What are these two sub-atomic particles called? n atom with a mass number of 12 is used as the reference when calculating relative atomic masses. Which element is this an atom of? carbon hydrogen lead D oxygen Ethanol is made in a reversible reaction form ethene and water. The equation is 2 H 4 + H 2 O 2 H 5 OH Which statement correctly describes the yield? D mass of ethanol and water mass of ethanol made mass of ethene reacted mass of reactants and products This resource sheet may have been changed from the original. 1
2 student calculated that the maximum theoretical mass of ethanol made in the reaction would be 90 g. In the practical the student actually made 60 g of ethanol. alculate the percentage yield. Give your answer to 2 significant figures. Use the equation percentage yield = mass of product actually made maximum theoretical mass of product Suggest one reason why the mass collected was less than expected. D ethanol is a liquid ethene is too reactive reversible reaction steam was used 0 4 alcium oxide is produced by heating calcium carbonate. The equation for the reaction is: ao 3 ao + O 2 Use the equation to calculate the atom economy for the production of calcium oxide. Relative formula mass of desired product from equation tom economy = 100 Sum of relative formula masses of all reactants from equations Relative formula masses: ao 3 = 100, ao = 56 This resource sheet may have been changed from the original. 2
3 Sodium hydroxide and sulfuric acid react together to produce sodium sulfate and water. alance the equation for the reaction.... NaOH + H 2 SO 4 Na 2 SO H 2 O In the reaction, how does the mass of the products compare with the mass of the reactants? student investigated the volume of sulfuric acid that reacted with 25 cm 3 sodium hydroxide. Describe a titration method the student could use in this investigation. [6 marks] student investigated the reaction of magnesium with oxygen. The student calculated that 4.8 g of magnesium oxide would make 8.0 g of magnesium oxide. The equation for the reaction is: 2Mg + O 2 2MgO What mass of oxygen is required to produce 8.0 g of magnesium oxide from 4.8 g of magnesium? This resource sheet may have been changed from the original. 3
4 The student heated magnesium to produce magnesium oxide. Figure 1 shows the apparatus the student used. Figure 1 The student: weighed 2.40 g of magnesium heated the crucible and magnesium when heating lifted up the lid slightly to let oxygen in but stopped magnesium oxide escaping heated until all the magnesium formed a white powder weighed the magnesium ribbon formed. Table 2 shows the student s results. Table 2 Trial 1 Trial 2 Trial 3 Trial 4 Mass of magnesium in g Mass of magnesium oxide in g alculate the mean mass of magnesium oxide produced. Give your answer to 2 decimal places This resource sheet may have been changed from the original. 4
5 The student produced less magnesium oxide than expected. Suggest two reasons why. student made two solutions solution and solution. Solution contained 5 g of copper sulfate in 50 cm 3 of water. Solution contains 10 g of copper sulfate in 100 cm 3 of water. The student added solution to solution. The student concluded that the new solution is more concentrated because it has more copper sulfate dissolved in it. Is the student correct? Explain your answer. This resource sheet may have been changed from the original. 5
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