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 1.5 Ideal gases Question Bank

[Maximum number: 1]

Chlorine undergoes many reactions.

(a)

2.67 g of manganese(IV) oxide was added to $200.0 \mathrm{~cm}^{3}$ of $2.00 \mathrm{moldm} \mathrm{m}^{-3} \mathrm{HCl}$ .

\mathrm{MnO}_{2}(\mathrm{~s})+4 \mathrm{HCl}(\mathrm{aq}) \rightarrow \mathrm{Cl}_{2}(\mathrm{~g})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})+\mathrm{MnCl}_{2}(\mathrm{aq})

[ 1 ]

(i)

Calculate the volume of chlorine, in $\mathrm{dm}^{3}$ , produced if the reaction is conducted at standard temperature and pressure (STP). Use section 2 of the data booklet.

[ 1 ]

[Maximum number: 2]

Lithium reacts with water to form an alkaline solution.

(a)

A0.200 g piece of lithium was placed in $500.0 \mathrm{~cm}^{3}$ of water.

[ 2 ]

(i)

Calculate the volume of hydrogen gas produced, in $\mathrm{cm}^{3}$ , if the temperature was $22.5^{\circ} \mathrm{C}$ and the pressure was 103 kPa . Use sections 1 and 2 of the data booklet.

[ 2 ]

[Maximum number: 1]

Phosphine (IUPAC name phosphane) is a hydride of phosphorus, with the formula $\mathrm{PH}_{3}$ .

(a)

2.478 g of white phosphorus was used to make phosphine according to the equation:

\mathrm{P}_{4}(\mathrm{~s})+3 \mathrm{OH}^{-}(\mathrm{aq})+3 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \rightarrow \mathrm{PH}_{3}(\mathrm{~g})+3 \mathrm{H}_{2} \mathrm{PO}_{2}^{-}(\mathrm{aq})

[ 1 ]

(i)

Determine the volume of phosphine, measured in $\mathrm{cm}^{3}$ at standard temperature and pressure, that was produced.

[ 1 ]

[Maximum number: 4]

Alkanes are commonly occurring organic compounds.

(a)

The first four straight chain alkanes are gases at room temperature.

Boiling points of straight chain alkanes

[ 4 ]

(i)

Calculate the volume, in $\mathrm{dm}^{3}$ , occupied by 6.45 g of propane gas at 100 kPa and $15^{\circ} \mathrm{C}$ .

[ 2 ]

(ii)

Outline why the volume occupied by propane(g) at very high pressure is higher than the value calculated using PV=nRT.

[ 2 ]

[Maximum number: 3]

Nitrogen monoxide, NO(g), is produced in internal combustion and jet engines.

(a)

Calculate the amount, in moles, of NO in $1.0 \times 10^{-3} \mathrm{~m}^{3}$ of engine exhaust gas which contains 0.10 % NO by volume at $200^{\circ} \mathrm{C}$ and $1.0 \times 10^{5} \mathrm{~Pa}$ .

Use sections 1 and 2 of the data booklet.

[ 3 ]

[Maximum number: 2]

A powder has the following percentage composition by mass:
30.0 % sucrose, $\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}$
45.0 % citric acid, $\mathrm{C}_{6} \mathrm{H}_{8} \mathrm{O}_{7}$
25.0 \% sodium hydrogencarbonate, $\mathrm{NaHCO}_{3}$

In the presence of water, the powder effervesces as the citric acid reacts with the sodium hydrogencarbonate:

$3 \mathrm{NaHCO}_{3}(\mathrm{~s})+\mathrm{C}_{6} \mathrm{H}_{8} \mathrm{O}_{7}(\mathrm{aq}) \rightarrow \mathrm{Na}_{3}\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{7}\right)(\mathrm{aq})+3 \mathrm{CO}_{2}(\mathrm{~g})+3 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})$

(a)

(i)

Determine the volume, in $\mathrm{dm}^{3}$ at SATP, of carbon dioxide released in the reaction in (a)(i). Use sections 1 and 2 of the data booklet.

[ 2 ]

[Maximum number: 2]

An organic compound, A, has the following composition by mass when its only combustion products, carbon dioxide and water, are analysed.

(a)

A sample of the vapour of A at $200.0^{\circ} \mathrm{C}$ and $1.00 \times 10^{5} \mathrm{~Pa}$ has a density of $2.544 \times 10^{3} \mathrm{~g} \mathrm{~m}^{-3}$ . Determine the molar mass and the molecular formula of A.

[ 2 ]

[Maximum number: 1]

The volume of a sample of gas measured at $27^{\circ} \mathrm{C}$ is $10.0 \mathrm{dm}^{3}$ . What is the temperature when the volume is reduced to $9.0 \mathrm{dm}^{3}$ at the same pressure?

$-3.0^{\circ} \mathrm{C}$

$24.3^{\circ} \mathrm{C}$

$29.7^{\circ} \mathrm{C}$

$57.0^{\circ} \mathrm{C}$

Which graph shows the relationship between the volume and pressure of a fixed mass of an ideal gas?

[Maximum number: 1]

The volume occupied by one mole of an ideal gas at 273 K and $1.01 \times 10^{5} \mathrm{~Pa}$ is $22.4 \mathrm{dm}^{3}$ . What volume, in $\mathrm{dm}^{3}$ , is occupied by $3.20 \mathrm{~g} \mathrm{O}_{2}(\mathrm{~g})$ at 273 K and $1.01 \times 10^{5} \mathrm{~Pa}$ ?

2.24

4.48

22.4

71.7

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