Pearson Edexcel International GCSE (9–1) · CHEMISTRY · Unit
Principles of Chemistry
991 practice questions
Topics covered
- States of Matter102 practice questions
- Elements, Compounds and Mixtures69 practice questions
- Atomic Structure108 practice questions
- The Periodic Table103 practice questions
- Chemical Formulae, Equations and Calculations Part 119 practice questions
- Chemical Formulae, Equations and Calculations Part 2144 practice questions
- Ionic Bonding143 practice questions
- Covalent Bonding68 practice questions
- Metallic Bonding19 practice questions
- Electrolysis198 practice questions
Practice questions
191–200 of 423 · Normal
Question 191
4 marks · Normal
Answer and see the solution →Hydrochloric acid reacts with sodium carbonate to produce sodium chloride, carbon dioxide and water. The balanced equation is:
(a)[2 marks]Calculate the number of moles in 1.06 g of sodium carbonate. (Ar: Na = 23, C = 12, O = 16)
(b)[2 marks]Calculate the volume, in dm³, of carbon dioxide produced at rtp by this mass of sodium carbonate. (Molar volume at rtp = 24 dm³)
Question 192
3 marks · Normal
Answer and see the solution →Calculate the number of moles in 360 cm³ of nitrogen gas at room temperature and pressure. Give your answer to two decimal places. (Molar volume = 24,000 cm³ at rtp)
Question 193
3 marks · Normal
Answer and see the solution →A student needs to calculate the mass of carbon dioxide produced when 48,000 cm³ of carbon dioxide is collected at room temperature and pressure. Explain the steps, including the formulae needed, to calculate the mass of carbon dioxide produced. (Ar: C = 12, O = 16; molar volume = 24,000 cm³ at rtp)
Question 194
4 marks · Normal
Answer and see the solution →The table below shows the volumes, in cm³, of a gas collected from several reactions at room temperature and pressure. Fill in the number of moles of gas for each row, using the molar volume of 24,000 cm³ at rtp.
Volume (cm³) Moles 6000 12,000 1800 24,000 Question 195
1 mark · Normal
Answer and check →Which calculation gives the number of moles of a gas from its volume at rtp (using cm³)?
- A.moles = volume / 24,000
- B.moles = mass / Mr
- C.moles = volume × 24,000
- D.moles = Mr / mass
Question 196
2 marks · Normal
Answer and see the solution →Calculate the volume, in dm³, of chlorine gas produced at rtp from the complete decomposition of 2.7 g of potassium chlorate, KClO₃. The balanced equation is:
(Ar: K = 39, Cl = 35.5, O = 16; molar volume = 24 dm³)
Question 197
4 marks · Normal
Answer and see the solution →Ammonium nitrate decomposes to form dinitrogen oxide (N2O) and water. The balanced equation is:
A practical uses 8.0 g of ammonium nitrate. (Ar: N = 14, H = 1, O = 16; molar volume at rtp = 24 dm³)
(a)[2 marks]Calculate the number of moles of ammonium nitrate used.
(b)[2 marks]Calculate the volume, in dm³, of dinitrogen oxide (N₂O) formed at rtp.
Question 198
2 marks · Normal
Answer and see the solution →A solution contains 4.0 g of potassium chloride (KCl) dissolved in exactly 100 cm³ of water. Calculate the concentration of this solution in g/dm³.
Question 199
4 marks · Normal
Answer and see the solution →(a)[1 mark]Give the formula that links concentration in mol/dm³, amount in mol, and volume in dm³.
(b)[1 mark]A student dissolves 2.5 g of magnesium sulfate (MgSO₄, Ar: Mg = 24, S = 32, O = 16) in 200 cm³ of water.
i. Calculate the number of moles of MgSO₄ in the solution.
(c)[2 marks]ii. Calculate the concentration of MgSO₄ in mol/dm³ in the solution.
Question 200
3 marks · Normal
Answer and see the solution →Calculate the mass of sodium nitrate (NaNO₃, Ar: Na = 23, N = 14, O = 16) required to make 250 cm³ of a 0.050 mol/dm³ solution.