Pearson Edexcel International GCSE (9–1) · CHEMISTRY · Chapter
Chemical Formulae, Equations and Calculations Part 2
144 practice questions
Topics covered
- Calculations involving gas volumes19 practice questions
- Calculating the volume of a certain number of moles19 practice questions
- Using the molar volume in calculations with chemical equations19 practice questions
- Concentrations of solutions19 practice questions
- Calculations with equations involving solutions19 practice questions
- The standard calculation19 practice questions
- Reversing the calculations20 practice questions
Practice questions
31–40 of 59 · Easy
Question 31
3 marks · Easy
Answer and see the solution →(a)A student wants to make 500 cm³ of a 0.08 mol/dm³ solution of calcium chloride (CaCl₂).
(i)[2 marks]Calculate the amount of CaCl₂ (in mol) needed.
(ii)[1 mark]State the volume, in dm³, of solution the student will prepare.
Question 32
2 marks · Easy
Answer and see the solution →A solution has a concentration of 0.25 mol/dm³. What volume of this solution (in cm³) contains 0.050 mol of solute? Show your answer to the nearest cm³.
Question 33
1 mark · Easy
Answer and see the solution →State the mass of sodium chloride, NaCl, produced when 0.025 mol of NaCl is formed in a reaction.
Question 34
3 marks · Easy
Answer and see the solution →A solution contains 0.30 mol/dm³ potassium chloride, KCl. 40 cm³ of this solution is measured out.
(a)[1 mark]Convert 40 cm³ to dm³.
(b)[2 marks]Calculate the number of moles of KCl in 40 cm³ of solution.
Question 35
2 marks · Easy
Answer and see the solution →The equation for a reaction is:
Calculate the number of moles of silver nitrate, AgNO₃, required to react with 0.030 mol of sodium carbonate, Na₂CO₃.
Question 36
2 marks · Easy
Answer and see the solution →A student adds 50 cm³ of 0.20 mol/dm³ hydrochloric acid, HCl, to excess calcium carbonate, CaCO₃.
The equation is:
Explain, using calculations, how to find the mass of CaCO₃ that will react with the HCl. Include your method and final answer. (Ar: Ca = 40, C = 12, O = 16)
Question 37
3 marks · Easy
Answer and see the solution →A student prepares solutions of nitric acid with different concentrations. The table shows the volume and concentration of nitric acid used in each experiment.
Volume and concentration data for nitric acid solutions. Experiment Volume (cm³) Concentration (mol/dm³) 1 25 0.20 2 40 0.10 3 50 0.16 Calculate the number of moles of nitric acid in each experiment. Give your answers to two decimal places.
(a)[1 mark]Experiment 1:
(b)[1 mark]Experiment 2:
(c)[1 mark]Experiment 3:
Question 38
1 mark · Easy
Answer and see the solution →The balanced equation for the reaction between hydrochloric acid and sodium carbonate is:
If 0.04 mol of sodium carbonate reacts completely, how many moles of hydrochloric acid are required to react with it?
Question 39
3 marks · Easy
Answer and see the solution →Zinc sulfate can be made by reacting zinc oxide with sulfuric acid as follows:
(a)[1 mark]25 cm³ of 0.20 mol/dm³ sulfuric acid is used in the reaction. Calculate the number of moles of sulfuric acid used.
(b)[1 mark]How many moles of zinc sulfate could be formed from this amount of sulfuric acid?
(c)[1 mark]Calculate the maximum mass of zinc sulfate, ZnSO₄ (Mᵣ = 161), formed.
Question 40
2 marks · Easy
Answer and see the solution →Calculate the number of moles of potassium chloride, KCl, dissolved in 15 cm³ of solution with a concentration of 0.25 mol/dm³.