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R2.1 How much? The amount of chemical change - IB Questionbank | RevisionDojo

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 2

Iron(III) oxide reacts with aluminum in a thermite reaction.

Identify the limiting reagent if $5.00\ \mathrm{g}$ of ${Fe_2O_3}$ and $3.00\ \mathrm{g}$ of ${Al}$ are used.

[2]

Calculate the theoretical mass of ${Fe}$ produced.

[2]

If $2.35\ \mathrm{g}$ of ${Fe}$ is collected, calculate the percentage yield.

[2]

Question 5

SLPaper 2

Caffeine is a stimulant commonly found in coffee and tea. Its molecular structure is shown below:

State the number of carbon atoms in the caffeine molecule that are part of a ring.

[1]

Identify the functional group(s) present in the caffeine molecule.

[1]

Deduce the molecular formula of caffeine from its displayed structure.

[1]

Caffeine is only sparingly soluble in water but is more soluble in ethanol.

Suggest why this is the case, referring to intermolecular forces.

[2]

The molar mass of caffeine is 194.19 $\text{g mol}^{-1}$ .

Calculate the mass of caffeine in $250 \text{ cm}^3$ of a $0.010 \text{ mol dm}^{-3}$ solution.

[2]

Question 6

SLPaper 2

Magnesium reacts with hydrochloric acid to produce a salt and hydrogen gas.

Write the balanced chemical equation with state symbols.

[1]

Calculate the mass of magnesium chloride produced from 0.12 g of magnesium.

[2]

State the mole ratio of ${Mg}$ to ${MgCl_2}$ in the equation.

[1]

Question 7

SLPaper 2

Water is produced by combustion of hydrogen.

Write a balanced chemical equation.

[1]

Calculate the atom economy for the production of water.

[2]

State one reason why atom economy is useful in green chemistry.

[1]

Question 8

SLPaper 2

Sodium reacts with chlorine to form sodium chloride.

Write a balanced chemical equation with state symbols.

[1]

Identify the limiting reactant when 2.30 g of ${Na}$ reacts with 3.20 g of ${Cl_2}$ .

[2]

Calculate the maximum mass of ${NaCl}$ that can be formed.

[2]

Question 9

SLPaper 2

Zinc reacts with dilute sulfuric acid according to the following equation:

$Zn(s)+H_2SO_4(aq) \to ZnSO_4(aq)+H_2(g)$

A student reacts $3.00\ \mathrm{g}$ of zinc with $25.0\ \mathrm{cm^3}$ of $1.00\ \mathrm{mol\ dm^{-3}}$ sulfuric acid.

Determine the limiting reactant in this reaction.

[2]

Calculate the volume of hydrogen gas produced at STP.

[2]

If the experiment yields 85% of the expected hydrogen gas, calculate the actual volume collected.

[1]

Question 10

SLPaper 2

Sodium hydroxide reacts with hydrochloric acid in a neutralization.

Write a balanced chemical equation for the reaction.

[1]

Calculate the concentration of ${NaOH}$ if $25.0\ \mathrm{cm^3}$ reacts with $25.0\ \mathrm{cm^3}$ of $0.100\ \mathrm{mol\ dm^{-3}}$ ${HCl}$ .

[2]

Determine the amount (mol) of water formed.

[1]

Structure 1. Models of the particulate nature of matter5 subtopics

Structure 2. Models of bonding and structure4 subtopics

Structure 3. Classification of matter2 subtopics

Reactivity 1. What drives chemical reactions?4 subtopics

Reactivity 2. How much, how fast and how far?3 subtopics

Reactivity 3. What are the mechanisms of chemical change?4 subtopics

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