igcse model questions vol1 2024 chemistry | Practical

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Question 1 View Details
A sample of a hydrated copper(II) sulphate is analysed by heating in a crucible until a constant mass is obtained. The data recorded are: - Initial mass of crucible + sample = 15.00 g - Mass of crucible + residue after heating = 12.20 g The residue is known to be anhydrous CuSO₄. Using the data provided, answer the following questions.
Question Parts
(a)
Calculate the mass of water lost on heating.
(b)
Determine the empirical formula of the original hydrate (CuSO₄·xH₂O). Show all calculations.
(c)
Calculate the percentage by mass of copper in the hydrate CuSO₄·5H₂O.
(d)
Suggest one possible source of error that could affect the calculated percentage of copper and explain how it would influence the result.
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Question 2 View Details
A colourless aqueous solution of an unknown metal chloride is examined using the following observations: 1. Flame test – a bright brick‑red colour is observed. 2. Adding dilute hydrochloric acid produces a steady stream of bubbles. 3. Adding a few drops of sodium carbonate solution results in the formation of a white precipitate. 4. The solution remains colourless throughout the tests. Using the observations above, answer the following questions.
Question Parts
(a)
Identify the metal ion present in the solution. Write its chemical symbol.
(b)
State the group number and period of the identified element in the modern periodic table.
(c)
Compare the first ionisation energy of the identified element with that of sodium (Na). State whether it is higher or lower and give a brief justification using periodic trends.
(d)
Suggest one practical precaution that should be taken when performing the flame test to avoid contamination of the result.
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Question 3 View Details
A student is investigating the composition of a metal oxide by the reduction method. The following masses were recorded: - Empty crucible: 10.00 g - Crucible + metal oxide before heating: 40.00 g - Crucible + metal after heating (all oxygen removed): 34.00 g The metal oxide is heated strongly in a reducing atmosphere until a constant mass is obtained.
Question Parts
(a)
Write the balanced chemical equation for the reduction of the metal oxide to the metal.
(b)
Calculate the mass of metal obtained after heating.
(c)
Using the data, determine the empirical formula of the original metal oxide.
(d)
State the type of chemical bonding present in the oxide you have identified and give one piece of evidence supporting your answer.
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Question 4 View Details
A student collects an unknown gas over water at 298 K. The following data are recorded: - Volume of gas collected (corrected to dry gas): 250.0 cm³ (0.250 L)\n- Atmospheric pressure: 760 mm Hg\n- Vapor pressure of water at 298 K: 23.8 mm Hg\n- Mass of the dry gas collected: 0.277 g\nThe gas is assumed to behave ideally.
Question Parts
(a)
Calculate the number of moles of gas collected.
(b)
Determine the molar mass of the unknown gas.
(c)
From the following options, identify the gas: (i) N₂, (ii) O₂, (iii) CO₂, (iv) H₂.
(d)
State two possible sources of error that could affect the calculated molar mass.
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