igcse model questions vol1 2025 chemistry | Practical

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Question 1 View Details
A student carries out the following experiment to determine the relative atomic mass of magnesium (Mg). A clean crucible with lid is weighed and the mass recorded as 15.842 g. An excess of magnesium ribbon is placed in the crucible and the crucible is re‑weighed. After heating the crucible strongly for 5 min the lid is replaced and the crucible is cooled in a desiccator and weighed again. The experiment is repeated a second time with a fresh crucible. The data obtained are shown in the table below. | Trial | Mass of empty crucible (g) | Mass of crucible + Mg before heating (g) | Mass of crucible + MgO after heating (g) | |-------|----------------------------|------------------------------------------|-------------------------------------------| | 1 | 15.842 | 18.376 | 19.621 | | 2 | 15.830 | 18.363 | 19.608 | Using the data, answer the following questions:
Question Parts
(a)
Calculate the mass of magnesium used in each trial.
(b)
From the data, determine the relative atomic mass of magnesium. Show all steps and give your final answer to the nearest whole number.
(c)
Identify two possible sources of error that could affect the accuracy of the experimental atomic mass obtained.
(d)
Suggest one improvement to the experimental procedure that would reduce the error identified in part (c).
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Question 2 View Details
A student is given an unknown metallic solid and is asked to identify it using density determination and periodic‑table data. The student measures the mass of the metal using an analytical balance and then determines its volume by water displacement in a graduated cylinder. The data recorded are shown below. | Measurement | Value | |-------------|-------| | Mass of metal (g) | 23.48 | | Initial water level (mL) | 45.0 | | Final water level after immersion (mL) | 51.3 | The periodic table data supplied to the class list the densities of several possible metals: - Aluminium: 2.70 g cm⁻³ - Copper: 8.96 g cm⁻³ - Iron: 7.87 g cm⁻³ - Zinc: 7.14 g cm⁻³ - Lead: 11.34 g cm⁻³ Using the experimental data and the table, answer the following:
Question Parts
(a)
Calculate the density of the unknown metal. Give your answer to three significant figures.
(b)
From the periodic‑table data, identify the most likely metal. Explain the basis of your choice.
(c)
List two sources of error that could cause the experimentally determined density to be higher than the true value.
(d)
Suggest one procedural improvement that would reduce the error identified in part (c).
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Question 3 View Details
You are given an unknown solid sample labelled X. The following experimental observations were recorded during a series of qualitative tests. Observations: - Solubility in water: dissolves completely, clear solution. - Solubility in ethanol: does not dissolve. - Conductivity of the aqueous solution (conductivity tester): high conductivity, 1.2 mS cm⁻¹. - Flame test: no characteristic colour observed. Using the data above, answer the questions that follow.
Question Parts
(a)
State the most probable type of chemical bonding present in sample X.
(b)
For each observation, explain how it supports the conclusion in part (a).
(c)
Suggest one additional experimental technique that could be used to confirm the type of bonding and outline the essential steps of the technique.
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Question 4 View Details
A volatile liquid of unknown identity was vaporised in a sealed eudiometer and the displaced gas was collected over water at 298 K. The data recorded are shown below. Data: - Mass of liquid weighed before vaporisation: 1.250 g - Atmospheric pressure: 760 mm Hg - Water vapour pressure at 298 K: 23.8 mm Hg - Temperature of the collected gas: 298 K - Volume of dry gas (corrected for water vapour): 0.400 L - Theoretical molar mass of the liquid (given): 78.1 g mol⁻¹ Using the information above, answer the following questions.
Question Parts
(a)
Calculate the number of moles of gas collected, correcting for the presence of water vapour.
(b)
Determine the experimental molar mass of the liquid.
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