National 5 Chemistry Unit 1 Practical Skills Past Paper Questions

1. Oxygen gas A. Burns with a pop B. Relights a glowing splint C. Turns damp pH paper red D. Turns limewater cloudy

2. The diagram below shows what happens when two solutions are mixed.

Which of the following terms describe the reaction that has taken place? A. Addition B. Neutralisation C. Precipitation D. Redox

3. The table contains information about calcium and calcium chloride.

When molten calcium chloride is electrolysed at 800 ºC the calcium appears as a

A. solid on the surface of the molten calcium chloride B. liquid on the surface of the molten calcium chloride C. solid at the bottom of the molten calcium chloride D. liquid at the bottom of the molten calcium chloride.

4. When hydrogen chloride gas is dissolved in water a solution containing hydrogen ions and chloride ions is formed. Which equation correctly shows the state symbols for this change?

5. The spectator ions in the reaction are

A. H+ (aq) and K+ (aq) - - B. NO3 (aq) and OH (aq) C. H+(aq) and OH-(aq) + - D. K (aq) and NO3 (aq)

6. Which of the following shows the metals in order of increasing reactivity? A. XYZ B. YXZ C. ZXY D. ZYX

7. Nitrogen dioxide is a brown coloured gas that is soluble in water and more dense than air. Which of the following diagrams shows the most appropriate method for collecting and measuring the volume of nitrogen dioxide?

8. A solution of a metal chloride burns with a green flame. Which of the following metal ions could be present in the metal chloride? You may wish to use the data booklet to help you. A. Ba2+ B. Ca2+ C. K+ D. Na+ 9. Which of the following salts can be prepared by a precipitation reaction? You may wish to use the data booklet to help you. A. Barium sulfate B. Lithium nitrate C. Calcium chloride D. Ammonium phosphate

10. A solution of accurately known concentration is more commonly known as a A. Correct solution B. Precise solution C. Standard solution D. Prepared solution

11. Read the passage below and attempt the questions that follow.

Hydrogen Storage The portable storage of hydrogen (H2) is key to the development of hydrogen fuel cell cars. While many chemists focus their attention on the use of metal alloys and hydrides for storing hydrogen, others have investigated the potential use of carbon nanotubes.

A carbon nanotube is a tiny rolled up sheet of graphite. A research team has designed a pillared structure made up of vertical columns of carbon nanotubes which stabilise parallel graphene sheets. Graphene sheets are layers of carbon which are one atom thick.

Lithium atoms are added to the pillared structure to increase the hydrogen storage capacity. Researchers claim that one litre of the structure can store 41 g of hydrogen gas, which comes close to the US Department of Energy’s target of 45 g.

Adapted from InfoChem Magazine (RSC), Nov 2008

a. Name the term used to describe a tiny rolled up sheet of graphite. (1) b. Name the metal added to the pillared structure to increase the hydrogen storage capacity. (1) c. Calculate the number of moles of hydrogen that, researchers claim, can be stored by one litre of this structure. (2)

12. Chlorine gas can be formed in the laboratory by adding concentrated hydrochloric acid to potassium permanganate. The gas is bubbled through water, to remove any unreacted hydrochloric acid, and then concentrated sulphuric acid to dry it. The chlorine gas is then collected in a gas jar.

Label the diagram for the preparation and collection of chlorine. (1)

13. A student was asked to carry out an experiment to determine the concentration of a copper (II) sulphate solution. Part of the work card used is shown.

a. Suggest how the student could have evaporated the solution to dryness. (1) 3 b. The student found that the 100 cm solution contained 3·19 g of copper(II) sulphate, CuSO4. Calculate the concentration of the solution in mol l –1. (3)

14. A student carried out an experiment to prepare the salt, magnesium sulphate.

Part of the experiment is shown below.

a. Name the acid used to make the salt. (1) b. How would the student know when to stop adding magnesium in Step 1? (1) c. Why was the reaction mixture filtered in Step 2? (1)

15. A student carried out an experiment to prepare the salt, magnesium chloride.

Part of the procedure is shown below.

Dry magnesium chloride crystals

Name steps 2 and 3 in the preparation of magnesium chloride. (2)

16. In the experiment, “Effect of temperature on reaction rate”, the reaction between sodium thiosulphate solution and dilute hydrochloric acid is investigated. The reaction was complete when the cross could no longer be seen as the reaction mixture turns cloudy.

a. How was the rate of reaction determined? (1) b. State a factor which should be kept constant. (1) c. Apart from wearing safety glasses, state another safety precaution which must be taken when carrying out this experiment. (1) d. The equation for the reaction taking place is

Rewrite the equation omitting the spectator ions. (1) 17. Egg shells are made up mainly of calcium carbonate. A pupil carried out an experiment to react egg shells with dilute hydrochloric acid. A gas was produced. a. Complete the diagram to show the apparatus which could have been used to measure the volume of gas produced. (1)

b. The volume of gas produced during the reaction was measured.

Plot these results as a graph. (4)

18. A student was asked to prepare the soluble compound, calcium propanoate. A section of the procedure used by the student is shown.

a. Write the formula, showing the charge on each ion, for calcium carbonate. (1) b. Complete the instruction for step 3 of the procedure. Continue adding the calcium carbonate until . . . (1) c. After step 3 has been completed a further two techniques are carried out to prepare a dry sample of calcium propanoate. Name the two techniques, in the correct order, that must be carried out. (1)

19. Sodium sulphate crystals can be made from sodium hydroxide solution and dilute sulphuric acid as shown in the procedure below.

Complete the instructions for step 1. (1)

20. In an experiment, a solution of copper (II) chloride was electrolysed.

a. What is meant by electrolysis? (1) b. Why is it necessary to use a d.c. supply in electrolysis? (1) c. Complete the table by adding the charge for each electrode. (1)