From Paper 1, Higher
Explain how iron is extracted from iron(III) oxide in a blast furnace and why carbon can be used.
From Paper 1, Higher
Describe how to prepare a pure, dry sample of copper(II) sulfate crystals from copper(II) oxide and dilute sulfuric acid.
From Paper 1, Higher
Predict the products at each electrode in the electrolysis of copper(II) chloride solution and write the half equation at the cathode.
From Paper 1, Higher
Explain why aluminium is extracted by electrolysis rather than reduction with carbon.
From Paper 1, Higher
Explain the difference between a strong acid and a weak acid.
From Paper 1, Higher
Explain the products of electrolysis of sodium chloride solution (brine).
From Paper 1, Higher
Write the ionic equation for the reaction of zinc with copper(II) sulfate and identify what is oxidised.
From Paper 1, Higher
The pH of an acid changes from 2 to 4. By what factor has the hydrogen ion concentration changed?
From Paper 1, Higher
Explain why ionic compounds must be molten or dissolved to be electrolysed.
From Paper 1, Higher
Describe an investigation to place four metals in order of reactivity using dilute acid.
From Paper 1, Higher
Write the ionic equation for neutralisation.
From Paper 1, Higher
In the electrolysis of aluminium oxide, the positive electrodes must be replaced regularly. Explain why.
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This paper is written by Plasmo in the style of the AQA GCSE Chemistry exam. It is not a past paper and is not produced or endorsed by the exam board.