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See if you can get 10 out of 10 in this Chemistry quiz.

Chemical Calculations (AQA Higher Tier)

For the GCSE Chemistry exam, you will be tested on calculations. In chemistry, we need to know how much of each reactant to use in order to make the right amount of product. Atoms are too small to count individually, so we weigh them instead.

Calculating the number of moles of a substance allows us to get the right ratio of our reactants for our reaction to work successfully. We also use calculations to help us decide how efficient our reactions are.

Atom economy is a way of quantifying how much waste there is associated with a particular reaction. Percentage yield is all important too. Chemists spend a long time working out the best conditions in order to maximise their yield.

Which of these compounds has the largest Mr?
Mr (which stands for Relative Formula Mass) is calculated by adding together all the atomic masses of the elements in the formula. In this case, rubidium is the heaviest group one atom mentioned so rubidium chloride will have the highest Mr. Which compound will have the lowest Mr?
The Mr of aluminium nitrate, Al(NO3)3 is…

(Ar: N - 14, O - 16, Al - 27)
When a formula contains brackets, anything inside the bracket needs to be multiplied by the number outside the bracket. So the formula for aluminium nitrate contains 1 aluminium atom, 3 nitrogen atoms and 9 oxygen atoms
Which of these reactions has an atom economy of 100%?
C2H4 + Br2 → C2H4Br2
CaCO3 → CaO + CO2
CaCO3 + HCl → CaCl2 + H2O + CO2
NaOH + HCl → NaCl + H2O
Atom economy is a measure of the environmental impact of a reaction. In an ideal world all or most of the reactants will end up in the product that you want. By definition, addition reactions like A have 100% atom economy because there is only one product. In industry, the atom economy of a reaction can be improved if a waste product can also be collected and sold. For example, the carbon dioxide made as waste in reactions B and C could be collected and sold to a fizzy drinks manufacturer
In the following reaction, if I fully react 400cm3 of methane, what volume of carbon dioxide should I expect to make?

CH4 + 2 O2 → CO2 + 2 H2O
100 cm3
200 cm3
300 cm3
400 cm3
One mole of any gas will occupy the same volume at a given temperature and pressure, regardless of what the gas is. In the above reaction 1 mole of methane reacts to form 1 mole of carbon dioxide, so the volume of carbon dioxide made will be the same as the volume of methane used
I make a solution of sodium hydroxide, NaOH, which has a concentration of 0.2 mol/dm3. What is its concentration in g/dm3?

Ar: Na: 23; O: 16; H: 1
200 g/dm3
40 g/dm3
8 g/dm3
0.2 g/dm3
The key to this question is not to over complicate it! It’s simply a case of converting a number of moles into a mass. Since mass = moles x Mr - the sum you need to do is 0.2 x Mr of NaOH
In the following reaction, if I fully react 4g of methane, what mass of water should I expect to make?

CH4 + 2 O2 → CO2 + 2 H2O
This is a reacting mass calculation. If you start with a known mass of a chemical, by using its Mr you can work out how many moles of it you have. In this case we have 0.25mol of methane. You can then use the stoichiometry of the reaction (aka the big balancing numbers!) to show you that every one mole of methane produces 2 moles of water. So we deduce that 0.5mol of water will be made. Then you simply need to use mass = moles x Mr to calculate the mass of water produced
In a titration I use 25cm3 of 0.20 mol/dm3 sodium hydroxide solution and find that it is neutralised by exactly 21cm3 of hydrochloric acid. What is the concentration of the hydrochloric acid solution?

HCl + NaOH → NaCl + H2O
9.5 mol/dm3
0.24 mol/dm3
0.19 mol/dm3
0.00024 mol/dm3
When doing this type of calculation, always start with the solution that you know most about – in this case the sodium hydroxide solution. Since you know both the volume and the concentration you can calculate how many moles of sodium hydroxide you have. Next look at the equation for the reaction; one mole of sodium hydroxide reacts exactly with one mole of hydrochloric acid. You therefore know how many moles of HCl there must have been in 21cm3 of solution. Since you know moles and volume, you can calculate the concentration
I make some ethyl ethanoate by reacting ethanol and ethanoic acid. Before carrying out the reaction I have calculated that I should be able to make 3.2g of my product. However, on weighing my purified product I find that I only have 1.8g. What is the percentage yield for my reaction?
Top tip: when calculating a percentage, if you get an answer greater than 100%, you definitely need to think again about your calculation. Any percentage is calculated by multiplying a fraction by 100. In this case you are finding what fraction of your expected yield you actually made, so the sum you need is 1.8/3.2 x 100
I dissolve 10g of NaOH in 100 cm3 of water. Which row shows the correct concentration in both g/dm3 and mol/dm3?
100 g/dm3; 2.5 mol/dm3
1 g/dm3; 0.025 mol/dm3
100 g/dm3; 0.4 mol/dm3
1 g/dm3; 4 mol/dm3
The first thing you need to do in this question is convert the volume in cm3 into dm3. Since there are 1000cm3 in a dm3, 100cm3 is 0.1 dm3. If you can’t remember how to calculate concentration, use the units to help you; grams per decimetre cubed means g divided by dm3, so the sum you need is 10 / 0.1. Then simply find out how many moles there are in 100g of NaOH. The RFM is 40 so the sum you need is 100/40
I have 2 dm3 of carbon dioxide gas at room temperature and pressure. How many moles do I have?
The key fact to remember here is that one mole of any gas occupies 24 dm3 at RTP. I have 1/12 of this volume, so I must have 1/12 of a mole
Author:  Kirstie Urquhart

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