Reactivity 2. How much, how fast and how far? Questionbank

Practice Reactivity 2. How much, how fast and how far? with authentic IB Chemistry exam questions for both SL and HL students. This question bank mirrors Paper 1A, 1B, 2 structure, covering key topics like atomic structure, chemical reactions, and organic chemistry. Get instant solutions, detailed explanations, and build exam confidence with questions in the style of IB examiners.

Paper

Level

Question 1

SLPaper 2

The reaction between sodium thiosulfate and hydrochloric acid forms a precipitate:

$\mathrm{Na_2S_2O_3(aq)} + 2\mathrm{HCl(aq)} \rightarrow 2\mathrm{NaCl(aq)} + \mathrm{S(s)} + \mathrm{SO_2(g)} + \mathrm{H_2O(l)}$

Describe a method to determine the rate of this reaction.

[2]

Suggest how temperature affects the time for the cross to disappear.

[1]

Explain this effect in terms of activation energy.

[2]

Question 2

SLPaper 2

Ethanol can be produced by fermentation of glucose under anaerobic conditions, a process widely used in the biofuel industry.

Write the balanced chemical equation for the fermentation of glucose, $C_6H_{12}O_6$ to produce ethanol.

[1]

Calculate the atom economy for ethanol in this process. (Give your answer to 1 decimal place.)

[2]

If $180\ \mathrm{g}$ of glucose is fermented, calculate the mass of ethanol and the mass of carbon dioxide produced.

[3]

Suggest one advantage and one disadvantage of using fermentation over industrial hydration of ethene.

[2]

Question 3

SLPaper 2

Carbon dioxide is collected from the decomposition of calcium carbonate.

Calculate the number of moles in 4.4 g of ${CO_2}$ .

[1]

Deduce the volume of this gas at STP.

[1]

Calculate the mass of ${CaCO_3}$ required to produce this amount of ${CO_2}$ .

[2]

Question 4

SLPaper 2

Ammonia is formed by the Haber process:

$N_2(g)+3H_2(g) \to 2NH_3(g)$

The diagram below shows the energy profile of this reaction.

State what is meant by the term activation energy.

[1]

Identify whether the reaction is exothermic or endothermic and justify your answer using the diagram.

[2]

Suggest one reason why a high temperature is required for this reaction to proceed at a practical rate.

[1]

Explain how the use of a catalyst would affect the energy profile diagram.

[2]

The Haber process is a reversible reaction. State and explain one condition used in industry to increase the yield of ammonia.

[2]

Question 5

SLPaper 2

Hydrogen peroxide decomposes slowly at room temperature:

$2\mathrm{H_2O_2(aq)} \rightarrow 2\mathrm{H_2O(l)} + \mathrm{O_2(g)}$

State one way to measure the rate of this reaction.

[1]

State how the rate of reaction changes as the reaction proceeds.

[1]

Explain your answer to part 2.

[2]

Question 6

SLPaper 1A

Several reactions of calcium carbonate with dilute hydrochloric acid are carried out at the same temperature.

$CaCO_3 (s) + 2HCl (aq) → CaCl_2 (aq) + H_2O (l) + CO_2 (g)$

Which reaction has the greatest rate?

Answer	Concentration of HCl(aq)	Surface area of same mass of CaCO₃(s)
A	higher	larger
B	lower	smaller
C	lower	larger
D	higher	smaller

Question 7

SLPaper 1A

The complete combustion of 15.0 $cm^3$ of a gaseous hydrocarbon X produces 60.0 $cm^3$ of carbon dioxide gas and 75.0 $cm^3$ of water vapour. What is the molecular formula of X? (All volumes are measured at the same temperature and pressure)

Question 8

HLPaper 1A

$MgCO_3(s) + 2HBr(aq) \rightarrow MgBr_2(aq) + H_2O(l) + CO_2(g)$

Which change does not increase the initial rate of reaction when $MgCO_3(s)$ is added to excess $HBr(aq)$ ?

Question 9

SLPaper 1A

How should a measurement of 5.00 g from a balance be recorded?

Question 10

HLPaper 1A

What volume of carbon dioxide, $CO_2$ (g), can be obtained by reacting 1 $dm^3$ of methane, $CH_4$ (g), with 1 $dm^3$ of oxygen, $O_2$ (g)?

$CH_4 (g) + 2O_2 (g) → CO_2 (g) + 2H_2O (l)$

Answer

Concentration of HCl(aq)

Surface area of same mass of CaCO₃(s)

higher

larger

lower

smaller

lower

larger

higher

smaller