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
931–940 of 991
Question 931
3 marks · Easy
Answer and see the solution →(a)[1 mark]Name the ion that will produce oxygen gas at the anode during the electrolysis of aqueous potassium sulfate solution with inert electrodes.
(b)[1 mark]Write the ionic equation for the formation of oxygen at the anode.
(c)[1 mark]State another negative ion commonly found in salts that will also result in the formation of oxygen at the anode.
Question 932
2 marks · Easy
Answer and see the solution →A student electrolyses an aqueous solution of potassium nitrate using inert electrodes.
State the name of the product formed at:
(a)[1 mark]the cathode
(b)[1 mark]the anode
Question 933
2 marks · Normal
Answer and see the solution →State the products formed at the cathode and at the anode when dilute sodium sulfate solution is electrolysed using inert electrodes.
Question 934
4 marks · Normal
Answer and see the solution →Potassium chloride solution is electrolysed using inert electrodes.
(a)[1 mark]State whether hydrogen or potassium is formed at the cathode.
(b)[2 marks]Explain why this product is formed at the cathode, using the reactivity series.
(c)[1 mark]Name the product formed at the anode.
Question 935
3 marks · Normal
Answer and see the solution →Electrolysis of aqueous copper(II) nitrate solution was carried out using inert electrodes. No copper was deposited at the cathode.
Explain which products are formed at the cathode and anode, and why these products are formed.
Question 936
4 marks · Normal
Answer and see the solution →The table shows part of the reactivity series and the likely product at the cathode during the electrolysis of an aqueous solution of the metal compound.
Metal Relative position (above/below H) Product at cathode Potassium Above Hydrogen Copper Below ? Sodium Above Hydrogen Silver Below ? a) Complete the column for 'Product at cathode' for copper and silver.
b) Explain, using the reactivity series, why these products are formed for copper and silver.
(a)[2 marks](b)[2 marks]Question 937
1 mark · Normal
Answer and check →Which of the following anions will produce oxygen gas at the anode, rather than a halogen, during electrolysis of an aqueous solution?
- A.Chloride (Cl⁻)
- B.Bromide (Br⁻)
- C.Sulfate (SO₄²⁻)
- D.Iodide (I⁻)
Question 938
2 marks · Normal
Answer and see the solution →Name the gases formed at the anode and at the cathode when dilute sulfuric acid is electrolysed with inert electrodes.
Question 939
4 marks · Normal
Answer and see the solution →A student electrolyses aqueous magnesium sulfate using inert electrodes.
(a)[1 mark]State the gas formed at the cathode.
(b)[2 marks]Explain why this product is formed at the cathode, using the reactivity series.
(c)[1 mark]Name the ion that is discharged at the anode.
Question 940
3 marks · Normal
Answer and see the solution →A student electrolyses an aqueous solution of sodium sulfate using inert electrodes.
She collects 120 cm³ of gas at the anode over a period of time.
Only two types of negative ions are present: sulfate ions and hydroxide ions.
State which ion is discharged at the anode, write the ionic equation for the reaction, and calculate the volume of oxygen molecules produced in moles (to 2 significant figures). (1 mol of any gas occupies 24 000 cm³ at room temperature and pressure.)
(a)[1 mark]State which ion is discharged at the anode.
(b)[1 mark]Write the ionic half-equation for the reaction at the anode.
(c)[1 mark]Calculate the amount of oxygen produced, in moles, to 2 significant figures.