CSEC Chemistry Paper 1 May/June 2008 - Free CXC Past Paper with Answers

It reacts with water to form a high concentration of hydrogen ions.

It reacts with water to form a low concentration of hydrogen ions.

It reacts with water to form a high concentration of hydroxide ions.

It reacts with water to form a low concentration of hydroxide ions.

It reacts with water to form a high concentration of hydrogen ions.

It reacts with water to form a low concentration of hydrogen ions.

It reacts with water to form a high concentration of hydroxide ions.

It reacts with water to form a low concentration of hydroxide ions.

$\text{HCl}$

$\text{NaOH}$

$\text{NaCl}$

$\text{H}_2\text{O}$

$\text{CO}_2$

$\text{CO}_3^{2-}$

$\text{HCO}_3^-$

$\text{OH}^-$

$\text{SO}_2$

$\text{CO}_2$

$\text{CaO}$

$\text{CO}$

$\text{MgO}$

$\text{Al}_2\text{O}_3$

$\text{Na}_2\text{O}$

$\text{SO}_3$

III only

I and II only

I, II and III only

I, III and IV only

A

B

C

D

atom

mole

formula

molecule

4

6

8

10

1

2

3

4

water and sodium chloride

water and ethanol

water and kerosene

kerosene and sodium chloride

use of a separating funnel

simple distillation

fractional distillation

sublimation

Magnesium

Aluminium

Sodium

Chlorine

I only

III only

I and II only

II and III only

solubility of product

TYPE of gas evolved

reaction with litmus

TYPE of product

The boiling point of the elements increases as their atomic numbers increase.

The oxidizing power of the elements decreases as their atomic numbers increase.

They are all nonmetals.

They form negative ions by the loss of electrons from their atoms.

react with zinc metal to produce hydrogen

react with zinc metal to produce a solution of pH 10

neutralize a solution of pH 4

react with hydrochloric acid to produce a salt and water

Salt

Base

Alkali

Acid

+4 / +2 / +4

-4 / +2 / +4

+4 / -2 / -4

-4 / +4 / +4

2SO₂(g) + O₂(g) → 2SO₃(g)

SO₂(g) + H₂O(l) → 2H₂O(l) + 3S(s)

SO₂(g) + H₂O(l) → H₂SO₄(aq)

SO₂(g) + 2HNO₃(aq) → H₂SO₄(aq) + 2NO₂(g)

aqueous copper (II) sulphate

copper

sulphur

sodium chloride

They contain molecules.

They are solids and vaporize easily.

They usually dissolve in organic solvents.

They conduct electricity when melted or dissolved in water.

The electrons leave the solution by the positive electrode.

Decomposition of the electrolyte at the electrode is due to an electric current.

The electrons enter the solution by the negative electrode.

Decomposition of the electrolyte at the electrode produces an electric current.

I

II

III

IV

as well as bond formation releases energy

requires less energy than is released when new bonds are formed

requires more energy than that released when new bonds are formed

is an endothermic process whereas bond making is an exothermic one

metallic ions

nonmetallic ions

spectator ions

radicals

I and II only

I and III only

II and III only

I, II and III

$\text{Cu}^{2+}(\text{aq})$ and $\text{SO}_4^{2-}(\text{aq})$

$\text{H}^+(\text{aq})$ and $\text{OH}^-(\text{aq})$

$\text{Cu}^{2+}(\text{aq})$ and $\text{H}^+(\text{aq})$

$\text{SO}_4^{2-}(\text{aq})$ and $\text{OH}^-(\text{aq})$

sodium is liberated at the cathode

the solution at the cathode is alkaline

oxygen is liberated at the anode

chlorine is liberated at the anode

carbon atoms in ethene are linked by single bonds.

molecule contains at least one double bond

carbon atoms in the molecule are very reactive

molecule has insufficient hydrogen atoms

$C_2H_6$

$C_4H_{10}$

$C_2H_4$

$C_3H_6$

$C_8H_{12}$

$C_8H_{14}$

$C_8H_{16}$

$C_8H_{18}$

I and II only

I and III only

II and III only

I, II and III

hydrogenation

addition polymerization

condensation polymerization

substitution

CH₃CH₂OH → CH₃COOH

CH₃CH₂OH → CH₃CHO

CH₃CH₂OH → C₂H₄

CH₃CH₂OH → 2CO₂ + 3H₂O

CH₃CH₂OH → CH₃COOH

CH₃CH₂OH → CH₃CHO

CH₃CH₂OH → C₂H₄

CH₃CH₂OH → 2CO₂ + 3H₂O

dilute hydrochloric acid

concentrated hydrochloric acid

dilute sulphuric acid

concentrated sulphuric acid

bitumen

paraffin oil

methane

propene

$C_6H_{12}O_6 + 6O_2 \rightarrow 6CO_2 + 6H_2O$

$C_6H_{12}O_6 + C_6H_{12}O_6 \rightarrow C_{12}H_{22}O_{11} + H_2O$

$C_6H_{12}O_6 \rightarrow 2C_2H_5OH + 2CO_2$

$6CO_2 + 6H_2O \rightarrow C_6H_{12}O_6 + 6O_2$

petroleum

methane

carbon

hydrogen

Fats

Starch

Proteins

Polyamides

Fats

Starch

Proteins

Polyamides

Polyalkene

Polyester

Polyamide

Polysaccharide

I and II only

I and III only

II and III only

III and IV only

addition polymerization

condensation polymerization

fermentation

vacuum distillation

III only

I and II only

II and III only

I, II and III

Carbon

Chlorine

Oxygen

Nitrogen

iron

nickel

platinum

vanadium (V) oxide

R, Q, P

P, Q, R

Q, R, P

R, P, Q

Aluminium is higher up in the activity series than iron, therefore it is more resistant to corrosion than iron.

Both metals form oxide coats but aluminium oxide prevents further reaction while the iron oxide does not.

Both metals form hydroxide coats but the aluminium hydroxide prevents further reaction while the iron hydroxide does not.

Aluminium is lower than iron in the activity series; therefore it reacts less readily with air than iron.

Calcium nitrate

Iron (II) nitrate

Copper (II) nitrate

Aluminium nitrate

$H_2S$

CaO

CO

$SO_2$

Sodium nitrate

Magnesium nitrate

Potassium nitrate

Copper (II) nitrate