(a) the number of CO2 molecules in 0.057 mol

(b) the number of atoms in 3 mol of N₂

(c) the number of O2 molecules in 1.5 mol.

(a) CO₂ and Br₂

(b) SO₃ and Cl₂

(a) Calculate the temperature of the air in the ball at the end of the match.

(b) Is it reasonable to assume that the volume of the ball remained constant? Explain your answer.

(c) If the volume of the ball is 0.400 dm3 , calculate the amount of air required to fill it before the game.

(a) Using the results, draw a sketch graph.

(b) Explain why the learner can deduce that the gas displays ideal gas behaviour in the experiment.

(c) Give the mathematical relationship in the experiment.

(d) Name the law that is illustrated in this experiment.

(a) Which set of properties of a gas must remain constant in an experiment to verify Boyle’s Law?

(b) A gas is collected and found to fill 4.73 cm3 at 35 °C. What will its volume be at standard temperature?

(c) 250 cm3 of hydrogen gas at a temperature of 17 °C are at a pressure of 196 kPa. Calculate the volume of hydrogen if the temperature is raised to 67 °C and the pressure is decreased to 80 kPa.

(d) The pressure of an empty aerosol can that originally contained air freshener is 108 kPa at 21 °C. The can has a volume of 400 cm3 . A boy throws this container into a fire and when the temperature and volume reach 210 °C and 410 cm3 respectively, it explodes. Calculate the pressure in the container just before the explosion.

(e) Calculate the volume at STP of a given mass of gas that occupies 200 dm3 at a pressure of 260 kPa and a temperature of −13 °C

(a) State which factors had to remain constant during this investigation.

(b) Calculate the value of X on the graph for trial A.

(c) Was trial B conducted at a higher or lower temperature than trial A?