20 cm3 0.5 mol dm-3), 2 g marble chips 2) Revise formulae and balanced equations. Check that students know how to work out the number of atoms of each element in a formula. CC8c Moles C1.52 Explain why, in a reaction, 1) When there are Students study the reaction Demonstrate the the mass of product large numbers of small between iron and copper formation of formed is controlled by items, people usually sulfate solution precipitates of lead the mass of the reactant find the number of iodide by adding which is not in excess them by measuring different volumes of The students should find C1.53 Deduce the stoichiometry their mass rather than lead nitrate solution that the correct balanced of a reaction from the counting e.g. cashiers to the same volume equation is masses of the reactants in banks check the of potassium iodide Fe + CuSO4 Cu + and products number of coins in a solution and use → C1.50 Recall that one mole of bag by finding their FeSO4 these to determine particles of a substance is mass. Have small, the mole ratio of lead Equipment: for each group defined as: sealed jars containing nitrate to potassium 100 cm3 beaker, a the Avogadro constant 1 mole of particles of iodide and hence the evaporating basin, eye number of particles (6.02 different substances balanced equation. protection, filter funnel with x 1023 atoms, molecules, e.g. 18g of water, 12g Tell the students that filter paper to fit, glass rod, formulae or ions) of that of carbon, 32g of equal volumes of the 25 cm3 measuring cylinder, substance sulfur, 56g of iron. solutions contain spatula, copper sulfate b substance mass of Explain that these equal numbers of solution ( 30 cm3 of ‘relative particle mass’ g each contain the same moles of the solutes. approximately 0.5 mol dm-3 C1.51 Calculate the number of: number of particles. The reaction is solution), distilled water, Ask the students to complete when the
20 cm3 0.5 mol dm-3), 2 g marble chips 2) Revise formulae and balanced equations. Check that students know how to work out the number of atoms of each element in a formula. CC8c Moles C1.52 C1.53 C1.50 C1.51 Explain why, in a reaction, the mass of product formed is controlled by the mass of the reactant which is not in excess Deduce the stoichiometry of a reaction from the masses of the reactants and products Recall that one mole of particles of a substance is defined as: a the Avogadro constant number of particles (6.02 x 1023 atoms, molecules, formulae or ions) of that substance b substance mass of ‘relative particle mass’ g Calculate the number of: 1) When there are large numbers of small items, people usually find the number of them by measuring their mass rather than counting e.g. cashiers in banks check the number of coins in a bag by finding their mass. Have small, sealed jars containing 1 mole of particles of different substances e.g. 18g of water, 12g of carbon, 32g of sulfur, 56g of iron. Explain that these each contain the same number of particles. Ask the students to Students study the reaction between iron and copper sulfate solution The students should find that the correct balanced equation is Fe + CuSO4 → Cu + FeSO4 Equipment: for each group 100 cm3 beaker, evaporating basin, eye protection, filter funnel with filter paper to fit, glass rod, 25 cm3 measuring cylinder, spatula, copper sulfate solution ( 30 cm3 of approximately 0.5 mol dm-3 solution), distilled water, Demonstrate the formation of precipitates of lead iodide by adding different volumes of lead nitrate solution to the same volume of potassium iodide solution and use these to determine the mole ratio of lead nitrate to potassium iodide and hence the balanced equation. Tell the students that equal volumes of the solutions contain equal numbers of moles of the solutes. The reaction is complete when the
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