igcse model questions vol1 2017 chemistry | Practical

Prepare for your exams with igcse model questions vol1 questions? Reviewing past/model questions is one of the most effective ways to guarantee a high score. This practice hub features authentic 2017 chemistry (Practical) questions designed to simulate the real exam environment.

Practice these randomly selected questions to test your readiness.

Question 1 View Details
You are given the following isotopic data for chlorine: | Isotope | Relative atomic mass (u) | Natural abundance (%) | |---------|--------------------------|-----------------------| | ^35Cl | 34.969 | 75.78 | | ^37Cl | 36.966 | 24.22 | Using this information, answer the questions below.
Question Parts
(a)
Calculate the relative atomic mass of chlorine to two decimal places.
(b)
Using the relative atomic mass obtained in part (a), calculate the number of moles present in a 0.250 g sample of chlorine gas (Cl₂). Give your answer in scientific notation to three significant figures.
(c)
State two possible sources of error that could affect the calculated relative atomic mass of chlorine in part (a).
Detailed Essay Solution & Marking Scheme Available

Get the step-by-step mathematical proofs, key points required by examiners, and a comprehensive breakdown from our AI Tutor.

Reveal Answer
Question 2 View Details
A flame test was carried out on a number of metal salts. The observed flame colours are recorded in the table below. | Sample (metal salt) | Observed flame colour | |----------------------|-----------------------| | Sodium chloride (NaCl) | Bright yellow | | Potassium chloride (KCl) | Lilac (pale violet) | | Calcium chloride (CaCl₂) | Brick‑red | | Barium chloride (BaCl₂) | Apple‑green | | Copper(II) sulphate (CuSO₄) | Blue‑green | Answer the following questions.
Question Parts
(a)
Identify the metal ion responsible for each observed flame colour.
(b)
Explain why a flame test produces characteristic colours for different metal ions.
(c)
The first ionisation energies are: Na = 496 kJ mol⁻¹, K = 419 kJ mol⁻¹. Using periodic trends, explain why potassium has a lower ionisation energy than sodium.
(d)
Predict which metal, sodium or potassium, would react more vigorously with cold water and justify your answer using periodic trends.
Detailed Essay Solution & Marking Scheme Available

Get the step-by-step mathematical proofs, key points required by examiners, and a comprehensive breakdown from our AI Tutor.

Reveal Answer
Question 3 View Details
Three unknown white solid samples are labelled A, B and C. The following experimental procedures are carried out on each sample: 1. Solubility test – a small amount of the solid is added to 20 mL of distilled water at room temperature. 2. Conductivity test – the resulting solution (if any) is placed between the electrodes of a conductivity tester. 3. Flame test – a clean nichrome wire is dipped into the solid and introduced into a non‑luminous Bunsen‑burner flame; any colour observed is recorded. The observations are recorded in the table below. | Sample | Solubility in water | Conductivity of solution | Flame colour | |--------|----------------------|--------------------------|--------------| | A | Dissolves completely | Conducts strongly | Green | | B | Does not dissolve | No conduction | No colour | | C | Dissolves sparingly | Weak conduction | No colour | Using the observations, answer the questions that follow.
Question Parts
(a)
State the observations for each sample as recorded in the table.
(b)
Identify the type of chemical bonding present in each sample (ionic, covalent or metallic) and give a brief justification based on the observations.
(c)
Suggest a plausible chemical formula for each sample, consistent with the type of bonding you have identified.
Detailed Essay Solution & Marking Scheme Available

Get the step-by-step mathematical proofs, key points required by examiners, and a comprehensive breakdown from our AI Tutor.

Reveal Answer
Question 4 View Details
A 0.845 g sample of an unknown hydrocarbon is burnt completely in excess oxygen in a combustion tube. The combustion products are passed through a series of traps and the following masses are collected: - Carbon dioxide (CO₂): 2.34 g\n- Water (H₂O): 0.945 g Using the data provided, answer the questions below.
Question Parts
(a)
Calculate the number of moles of carbon and hydrogen present in the original sample and determine its empirical formula.
(b)
The molar mass of the hydrocarbon is known to be 58 g mol⁻¹. Determine the molecular formula of the compound.
(c)
Calculate the number of molecules present in the original 0.845 g sample.
Detailed Essay Solution & Marking Scheme Available

Get the step-by-step mathematical proofs, key points required by examiners, and a comprehensive breakdown from our AI Tutor.

Reveal Answer

Master the Exam!

You've seen a preview, but there are thousands more questions plus AI tutor to break down complex solutions.

Unlock Full Access Available for Android & Windows
Help others prepare! Share this practice hub:
Chat with Support