Reacting Masses 1 of 24 Boardworks Ltd 2016
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1 Reacting Masses 1 of 24 Boardworks Ltd 2016
2 Reacting Masses 2 of 24 Boardworks Ltd 2016
3 What is a mole? 3 of 24 Boardworks Ltd 2016 A mole is an SI unit that is used to denote the number of atoms or molecules in a given amount of substance. A mole is defined as the number of atoms in exactly 12g of carbon-12. Moles can be used to balance equations and calculate the mass of reactants and products. The number of moles in a sample is calculated using this equation: number of moles (mol) = mass of substance (g) molar mass (g/mol)
4 Molar mass 4 of 24 Boardworks Ltd 2016 The molar mass is the mass in grams of one mole of a substance. For elements, this is simply the relative atomic mass (r.a.m) value in grams/mol. For compounds, the molar mass is equal to the relative formula mass (r.f.m) value in grams/mol. relative atomic mass Some elements exist as molecules, for example, O 2. The relative formula mass will need to be used for these elements rather than the atomic mass.
5 Calculations using Avogadro s constant 5 of 24 Boardworks Ltd 2016 The number of particles (atoms or molecules) of a substance can be calculated using Avogadro s constant. The number of particles in a substance can be calculated by: number of particles = moles x Avogadro s constant How many atoms are in 10g of aluminium (Al)? molar mass of Al = r.a.m = 27 moles of Al = mass molar mass = = moles number of atoms in moles of aluminium: 6.02 x x 0.370moles = 2.23 x atoms
6 The stoichiometric coefficient 6 of 24 Boardworks Ltd 2016 The stoichiometric coefficient is the number in front of each reactant and product in a chemical equation. It is not necessary to write a stoichiometric coefficient of 1, and so the equation becomes: The coefficient balances the number of atoms on both the reactant and product sides of the equation.
7 Using moles to balance equations (I) 7 of 24 Boardworks Ltd 2016 The stoichiometric coefficients can be determined using the known masses of reactants and products: Step 1: Write the unbalanced equation for the reaction Step 2: Use the given mass values to calculate the number of moles for each reactant and product. Step 3: Convert the moles into simple, whole number ratios. Step 4: Write out the balanced equation using the whole number ratio values.
8 8 of 24 Boardworks Ltd 2016 Using moles to balance equations (II) 54g of Aluminium (Al) reacts with 159 g of Iron(III) Oxide (Fe 2 O 3 )to produce 111g of Iron (Fe) and 101g of Aluminium Oxide (Al 2 O 3 ). What is the balanced equation for this reaction? Step 1: Write the equation for the reaction Step 2: Use the given mass values to calculate the number of moles for each reactant and product. moles of Al = = 2 mol moles of Fe 2 O 3 = = 0.99 = 1 mol moles of Fe = = 1.98 = 2 mol moles of Al 2 O 3 = = 0.99 = 1 mol
9 Using moles to balance equations (III) 9 of 24 Boardworks Ltd 2016 Step 3: Convert the moles into simple whole number ratios. Al : Fe 2 O 3 : Fe : Al 2 O 3 2 : 1 : 2 : 1 2 moles of aluminium react with 1 mole of iron oxide to produce 2 moles of iron, and 1 mole of aluminium oxide. Step 4: Write out the balanced equation using the whole number ratio values.
10 Limiting reactants 10 of 24 Boardworks Ltd 2016 The amount of product formed in a reaction will depend on the limiting reactant. This is the reactant that runs out first, bringing the reaction to an end. The other reactant(s) are said to be in excess. This means that there will be some left after the reaction.
11 Limiting reactants and balanced equations 11 of 24 Boardworks Ltd 2016 You can use balanced equations to identify limiting reactants. For example, if 2 moles of aluminium are reacted with 5 moles of iron oxide, which is the limiting reactant? From the equation we know that 2 moles of aluminium react with 1 mole of iron oxide. This means that 4 moles of iron oxide will be left (5-1=4). The iron oxide is in excess and the aluminium is the limiting reactant.
12 Reacting Masses 12 of 24 Boardworks Ltd 2016
13 What s the mass? 13 of 24 Boardworks Ltd 2016 If 28 g of iron reacts with excess copper sulfate solution, what mass of copper will be made? Two different methods can be used to answer this question: Remember: number of moles = mass of substance molar mass
14 Using relative atomic mass 14 of 24 Boardworks Ltd 2016 Working out reacting masses using relative atomic mass: Step 1: Write a balanced equation for the reaction. Step 2: Write down the relative atomic mass(r.a.m) or relative formula mass(r.f.m) of the reactants and products. Step 3: Multiple the r.a.m or r.f.m by the stoichiometric coefficient (the large number before each substance in the equation). Step 4: Use the balanced equation to write down the ratios of reactants and products. Step 5: Convert this into a ratio of reacting masses. Step 6: Multiply the ratio by the known mass (from the question).
15 Using RAM: worked example (1) 15 of 24 Boardworks Ltd 2016 If 28g of iron reacts with excess copper sulphate solution, what mass of copper will be made? Step 1: Write a balanced equation for the reaction: Step 2: Write down the relevant r.a.m: Fe = 56, Cu = 64 Cu:Fe = 1:1
16 Using RAM: worked example (2) 16 of 24 Boardworks Ltd 2016 Step 5: Convert to ratio of reacting masses. Ratio of Cu to Fe = 1:1 = 64 g : 56 g = Step 6: Multiply the ratio by the known mass (from the question). mass of Cu formed = 28g x = 32 g of Cu
17 Reacting masses and scale factors 17 of 24 Boardworks Ltd 2016
18 Using moles 18 of 24 Boardworks Ltd 2016 How do you work out reacting masses using moles? Step 1: Write a balanced equation for the reaction. Step 2: Turn the given mass value into the number of moles. Step 3: Use the balanced equation to work out the number of moles of the unknown substance. Step 4: Convert moles into mass using the formula: moles = mass molar mass This is rearranged to give: mass = moles molar mass moles mass molar mass
19 Using moles: worked example (1) 19 of 24 Boardworks Ltd 2016 If 28 g of iron reacts with excess copper sulfate solution, what mass of copper will be made? Step 1: Write a balanced equation for the reaction: Step 2: Turn the mass of iron into moles of iron:
20 Using moles: worked example (2) 20 of 24 Boardworks Ltd mole of Fe makes 1 mole of Cu mass = moles r.a.m = = 32g of Cu
21 Using moles in calculations 21 of 24 Boardworks Ltd 2016
22 Reacting Masses 22 of 24 Boardworks Ltd 2016
23 Glossary 23 of 24 Boardworks Ltd 2016
24 Multiple-choice quiz 24 of 24 Boardworks Ltd 2016
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