1. States of matter

1.1 Solids, liquids and gases

1.2 Diffusion

2. Atoms, elements and compounds

2.1 Elements, compounds and mixtures

2.2 Atomic structure and the Periodic Table

2.3 Isotopes

2.4 Ions and ionic bonds

2.5 Simple molecules and covalent bonds

2.6 Giant covalent structures

2.7 Metallic bonding

3. Stoichiometry

3.1 Formulae

3.2 Relative masses of atoms and molecules

3.3 The mole and the Avogadro constant

4. Electrochemistry

4.1 Electrolysis

4.2 Hydrogen–oxygen fuel cells

5. Chemical energetics

5.1 Exothermic and endothermic reactions

6. Chemical reactions

6.1 Physical and chemical changes

6.2 Rate of reaction

6.3 Reversible reactions and equilibrium

6.4 Redox

7. Acids, bases and salts

7.1 The characteristic properties of acids and bases

7.2 Oxides

7.3 Preparation of salts

8. The Periodic Table

8.1 Arrangement of elements

8.2 Group I properties

8.3 Group VII properties

8.4 Transition elements

8.5 Noble gases

9. Metals

9.1 Properties of metals

9.2 Uses of metals

9.3 Alloys and their properties

9.4 Reactivity series

9.5 Corrosion of metals

9.6 Extraction of metals

10. Chemistry of the environment

10.1 Water

10.2 Fertilisers

10.3 Air quality and climate

11. Organic chemistry

11.1 Formulae, functional groups and terminology

11.2 Naming organic compounds

11.3 Fuels

11.4 Alkanes

11.5 Alkenes

11.6 Alcohols

11.7 Carboxylic acids

11.8 Polymers

12. Experimental techniques and chemical analysis

12.1 Experimental design

12.2 Acid–base titrations

12.3 Chromatography

12.4 Separation and purification

12.5 Identification of ions and gases

IGCSE Chemistry 5.1 Exothermic and endothermic reactions Question Bank

[Maximum number: 1]

The diagrams show four pieces of laboratory equipment.

Which equipment is essential to find out if dissolving a salt in water is an exothermic process?

balance

pipette

stop-clock

thermometer

✓

$\boldsymbol{\chi}$

$\boldsymbol{\times}$

✓

$\boldsymbol{\chi}$

✓

$\boldsymbol{\chi}$

✓

$\boldsymbol{\times}$

[Maximum number: 1]

The diagrams show four pieces of laboratory equipment.

Which equipment is essential to find out if dissolving a salt in water is an exothermic process?

balance

pipette

stop-clock

thermometer

$\boldsymbol{\chi}$

✓

$\boldsymbol{\chi}$

✓

$\boldsymbol{\times}$

✓

$\boldsymbol{\chi}$

✓

$\boldsymbol{\times}$

[Maximum number: 1]

The diagrams show four pieces of laboratory equipment.

stop-clock

thermometer

Which equipment is essential to find out if dissolving a salt in water is an exothermic process?

balance

pipette

stop-clock

thermometer

$\boldsymbol{\chi}$

✓

$\boldsymbol{\chi}$

✓

$\boldsymbol{\times}$

✓

$\boldsymbol{\chi}$

✓

$\boldsymbol{\chi}$

✓

$\boldsymbol{\chi}$

[Maximum number: 1]

Solid R reacted with dilute sulfuric acid.

The initial temperature of the dilute sulfuric acid and the final temperature of the solution are shown.

initial temperature of the dilute sulfuric acid $\left({ }^{\circ} \mathrm{C}\right)$

What was the change in temperature in ${ }^{\circ} \mathrm{C}$ ?

-6

-4

[Maximum number: 6]

Period 3 contains the elements sodium to argon. This question asks about the chemistry of each of the Period 3 elements or their compounds.

(a)

Sulfur tetrafluoride, $\mathrm{SF}_{4}$ , can be made by combining gaseous sulfur with fluorine.

\mathrm{S}(\mathrm{~g})+2 \mathrm{~F}_{2}(\mathrm{~g}) \rightarrow \mathrm{SF}_{4}(\mathrm{~g})

The reaction is exothermic.

[ 6 ]

(i)

Complete the energy level diagram for this reaction. Include an arrow which clearly shows the energy change during the reaction.

[ 3 ]

(ii)

During the reaction the amount of energy given out is $780 \mathrm{~kJ} / \mathrm{mol}$ .

The F-F bond energy is $160 \mathrm{~kJ} / \mathrm{mol}$ .
Use this information to determine the bond energy, in kJ / mol, of one S-F bond in $\mathrm{SF}_{4}$ .

[ 3 ]

[Maximum number: 1]

Which reaction pathway diagram represents an endothermic reaction?

[Maximum number: 1]

The energy level diagram for a chemical reaction is shown.

Which statement about this reaction is correct?

The reaction is endothermic and energy is given out to the surroundings.

The reaction is endothermic and energy is taken in from the surroundings.

The reaction is exothermic and energy is given out to the surroundings.

The reaction is exothermic and energy is taken in from the surroundings.

[Maximum number: 1]

Ethene gas, $\mathrm{C}_{2} \mathrm{H}_{4}$ , is completely burned in excess oxygen to form carbon dioxide and water. The equation for this exothermic reaction is shown.

\mathrm{C}_{2} \mathrm{H}_{4}+3 \mathrm{O}_{2} \rightarrow 2 \mathrm{CO}_{2}+2 \mathrm{H}_{2} \mathrm{O}

The table shows the bond energies involved in the reaction.

What is the total energy change in this reaction?

$-954 \mathrm{~kJ} / \mathrm{mol}$

$-1010 \mathrm{~kJ} / \mathrm{mol}$

$-1313 \mathrm{~kJ} / \mathrm{mol}$

$-1369 \mathrm{~kJ} / \mathrm{mol}$

[Maximum number: 1]

Chlorine reacts with ethane to produce chloroethane and hydrogen chloride.

The reaction is exothermic.

The bond energies are shown in the table.

What is the energy change for the reaction?

$-1420 \mathrm{~kJ} / \mathrm{mol}$

$-120 \mathrm{~kJ} / \mathrm{mol}$

$+120 \mathrm{~kJ} / \mathrm{mol}$

$+1420 \mathrm{~kJ} / \mathrm{mol}$

[Maximum number: 1]

Hydrogen burns in oxygen.
The equation for the reaction is shown.

2 \mathrm{H}_{2}+\mathrm{O}_{2} \rightarrow 2 \mathrm{H}_{2} \mathrm{O}

The table shows the bond energies involved.

What is the energy given out during the reaction?

$-3226 \mathrm{~kJ} / \mathrm{mol}$

$-884 \mathrm{~kJ} / \mathrm{mol}$

$-486 \mathrm{~kJ} / \mathrm{mol}$

$-442 \mathrm{~kJ} / \mathrm{mol}$

0 selected

Question 2

Question 2

Question 2

Question 3

Question 2

Question 2(f)

Question 2(f)(i)

Question 2(f)(ii)

Question 10

Question 11

Question 11

Question 11

Question 11