Paper 2, Higher

Explain why the reactivity of Group 1 metals increases down the group.

Explain why powdered calcium carbonate reacts faster with acid than lumps of the same mass.

Compare hydrogen fuel cells with rechargeable batteries for powering cars.

Explain why the concentration of carbon dioxide in the atmosphere increased over the last 200 years.

Describe the reactions of ethanol: combustion, oxidation and with sodium.

The theoretical yield of a reaction is 12.0 g. The actual yield is 8.5 g. Calculate the percentage yield and give one reason why it is less than 100%.

Which substance has a giant covalent structure?

Which element is in Group 7?

Explain how to find the rate of reaction at a particular time from a graph of volume of gas against time.

Describe how to investigate the temperature change when different masses of a metal powder are added to copper(II) sulfate solution.

Explain how particulates in the air affect human health and the climate.

Compare addition and condensation polymerisation.

The theoretical yield of a reaction is 40.0 g. The actual yield is 34.2 g. Calculate the percentage yield and give one reason why it is less than 100%.

Describe the structure of graphene and fullerenes and give a use of each.

Predict the state and colour of astatine at room temperature, explaining your answer.

Explain why the rate of reaction decreases as a reaction proceeds.

Explain why a simple cell produces a voltage.

Describe a test to show that a gas is oxygen and explain why the early atmosphere contained little oxygen.

Write a balanced equation for the complete combustion of propane, C₃H₈.

5.85 g of solute is dissolved to make 250 cm³ of solution. Calculate the concentration in g/dm³.

Draw a dot-and-cross diagram for a water molecule and describe the bonding.

Explain why the reactivity of Group 7 elements decreases down the group.

A student measures the loss of mass when marble chips react with acid. Describe the method and how to calculate the rate.

Explain why combustion reactions need to be started with a spark or flame even though they are exothermic.

What is the general formula of alkanes?

4.0 g of solute is dissolved to make 500 cm³ of solution. Calculate the concentration in g/dm³.

Work out the formula of the ionic compound formed between aluminium ions (Al³⁺) and oxide ions (O²⁻).

Write the balanced equation for the reaction of sodium with chlorine.

Explain why catalysts are important in industry.

Write the overall equation for a hydrogen fuel cell.

Name the ester formed from ethanol and ethanoic acid and give two uses of esters.

25.0 cm³ of sodium hydroxide solution was neutralised by 20.0 cm³ of 0.150 mol/dm³ hydrochloric acid. Calculate the concentration of the sodium hydroxide in mol/dm³. NaOH + HCl → NaCl + H₂O

Explain the limitations of dot-and-cross and ball-and-stick models.

Explain why elements in the same group have similar chemical properties.

Explain why the temperature change in a neutralisation experiment may be less than expected and how to improve accuracy.

Explain why burning hydrocarbons in a limited supply of oxygen is dangerous.

Calculate the volume of hydrogen gas at room temperature and pressure produced when 0.48 g of magnesium reacts with excess acid. Mg + 2HCl → MgCl₂ + H₂ (1 mole of gas occupies 24 dm³)