Structure 1. Models of the particulate nature of matter

1.1 Introduction to the particulate nature of matter

1.2 The nuclear atom

1.3 Electron configurations

1.4 The mole

1.5 Ideal gases

Structure 2. Models of bonding and structure

2.1 The ionic model

2.2 The covalent model

2.3 The metallic model

2.4 From models to materials

Structure 3. Classification of matter

3.1 The periodic table

3.2 Functional groups: Organic compounds

Reactivity 1. What drives chemical reactions?

1.1 Measuring enthalpy changes

1.2 Energy cycles

1.3 Energy from fuels

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

2.1 Amount of chemical change

2.2 Rate of chemical change

2.3 Extent of chemical change

Reactivity 3. What are the mechanisms of chemical change?

3.1 Proton transfer reactions

3.2 Electron transfer reactions

3.3 Electron sharing reactions (Radicals)

3.4 Electron-pair sharing reactions

IB Chemistry SL 1.3 Energy from fuels Question Bank

[Maximum number: 1]

Which hydrocarbon would produce equal numbers of moles of $\mathrm{CO}_{2}$ and $\mathrm{H}_{2} \mathrm{O}$ upon complete combustion?

$\mathrm{CH}_{4}$

$\mathrm{C}_{2} \mathrm{H}_{2}$

$\mathrm{C}_{3} \mathrm{H}_{8}$

$\mathrm{C}_{4} \mathrm{H}_{8}$

[Maximum number: 1]

Ethyne, $\mathrm{C}_{2} \mathrm{H}_{2}$ , reacts with oxygen in welding torches.

(a)

Write an equation for the complete combustion of ethyne.

[ 1 ]

[Maximum number: 2]

Urea, $\left(\mathrm{H}_{2} \mathrm{~N}\right)_{2} \mathrm{CO}$ , is excreted by mammals and can be used as a fertilizer.

(a)

The combustion of urea produces water, carbon dioxide and nitrogen.

Formulate a balanced equation for the reaction.

[ 2 ]

[Maximum number: 1]

What is the sum of the integer coefficients when propene undergoes complete combustion?

-\mathrm{C}_{3} \mathrm{H}_{6}(\mathrm{~g})+\ldots \mathrm{O}_{2}(\mathrm{~g}) \rightarrow \underline{\hspace{1.8em}} \mathrm{CO}_{2}(\mathrm{~g})+\underline{\hspace{0.9em}} \mathrm{H}_{2} \mathrm{O}(\mathrm{l})

[Maximum number: 1]

The equation for the complete combustion of propene, $\mathrm{C}_{3} \mathrm{H}_{6}$ , is shown below.

2 \mathrm{C}_{3} \mathrm{H}_{6}(\mathrm{~g})+9 \mathrm{O}_{2}(\mathrm{~g}) \rightarrow 6 \mathrm{CO}_{2}(\mathrm{~g})+6 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})

Which mixture, when ignited, will lead to incomplete combustion and the formation of CO(g) ?

$2 \mathrm{dm}^{3}$ of propene and $10 \mathrm{dm}^{3}$ of oxygen

$0.5 \mathrm{dm}^{3}$ of propene and $2.3 \mathrm{dm}^{3}$ of oxygen

$1 \mathrm{dm}^{3}$ of propene and $4 \mathrm{dm}^{3}$ of oxygen

$3 \mathrm{dm}^{3}$ of propene and $14 \mathrm{dm}^{3}$ of oxygen

[Maximum number: 2]

Benzoic acid, $\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}$ , is another derivative of benzene.

(a)

(i)

Formulate the equation for the complete combustion of benzoic acid in oxygen using only integer coefficients.

[ 2 ]

[Maximum number: 2]

Methanoic acid can be produced by the hydrogenation of carbon dioxide according to the equilibrium

\mathrm{CO}_{2}(\mathrm{~g})+\mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{HCOOH}(\mathrm{~g})

(a)

Explain why this process has been extensively investigated in recent years.

[ 2 ]

[Maximum number: 1]

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

\left(M_{\mathrm{r}} \text { for ethanol }=46.0, \Delta H_{\mathrm{c}}^{\ominus}=-1367 \mathrm{~kJ} \mathrm{~mol}^{-1}\right)

$\frac{683.5}{1367 \times 46.0}$

$\frac{1367}{683.5 \times 46.0}$

$\frac{683.5 \times 46.0}{1367}$

$\frac{1367 \times 46.0}{683.5}$

[Maximum number: 2]

The open-chain structure of D-fructose is shown below.

(a)

State a balanced equation for the complete combustion of D-fructose.

[ 2 ]

[Maximum number: 1]

The following shows some compounds which can be made from ethene, $\mathrm{C}_{2} \mathrm{H}_{4}$ .

\text { ethene }\left(\mathrm{C}_{2} \mathrm{H}_{4}\right) \rightarrow \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{Cl} \rightarrow \mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O} \rightarrow \mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}

(a)

(i)

Write an equation for the complete combustion of the organic product in (b).

[ 1 ]

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Question 1

Question 1

Question 1(a)

Question 1

Question 1(f)

Question 2

Question 3

Question 2

Question 2(b)

Question 2(b)(ii)

Question 2

Question 2(a)

Question 13

Question 4

Question 4(d)

Question 3

Question 3(c)

Question 3(c)(i)