R2.1 How much? The amount of chemical change Questionbank

Practice R2.1 How much? The amount of chemical change 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

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 2

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 3

SLPaper 2

In a laboratory experiment, 1.20 g of product was obtained from a reaction with a theoretical yield of 1.50 g.

Define the term percentage yield.

[1]

Calculate the percentage yield.

[2]

State one reason why the yield may be lower than expected.

[1]

Question 4

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 5

SLPaper 1A

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

Question 6

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)?

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

Question 7

SLPaper 1A

What is the percentage yield when 7 g of ethene produces 6 g of ethanol?

$M_r$ (ethene) = 28 and $M_r$ (ethanol) = 46

$C_2H_4(g) + H_2O(g) → C_2H_5OH(g)$

Question 8

SLPaper 1A

What is the sum of the coefficients when the following equation is balanced using the smallest whole numbers?

$...C_6H_{12}O_6 (aq) → ...C_2H_5OH (aq) + ...CO_2 (g)$

Question 9

SLPaper 1A

Consider that $200.0 \mathrm{~cm}^{3}$ of a $0.75 \, \mathrm{mol \, dm}^{-3}$ solution of $\mathrm{BaCl}_{2}$ is added to $100.0 \, \mathrm{~cm}^{3}$ of a $0.10 \, \mathrm{mol \, dm}^{-3}$ solution of $\mathrm{Na}_{2} \mathrm{SO}_{4}$ . As a consequence, a precipitate of $\mathrm{BaSO}_{4}$ is formed as outlined in the equation below.

$\mathrm{BaCl}_{2}(\mathrm{aq})+\mathrm{Na}_{2} \mathrm{SO}_{4}(\mathrm{aq}) \rightarrow \mathrm{BaSO}_{4}(\mathrm{s})+2 \mathrm{NaCl}(\mathrm{aq})$

What is the amount, in mol, of $\mathrm{BaSO}_{4}$ produced?

Question 10

HLPaper 1A

Which expression gives the mass, in g , of ethanol required to produce 683.5 kJ of heat upon complete combustion?

$(M_r \text{ for ethanol} = 46.0, \Delta H_c^\ominus = -1367 \text{ kJ mol}^{-1})$