ReallyAcademics
IAL EDEXCEL CHEMISTRY UNIT 4 ALL
MULTIPLE CHOICE QUESTIONS BY TOPIC
PREFACE
There will 2 versions of Unit 4 past papers:
Sorted by Year
Sorted by Topic
I will also make a complete revision guide for A2 chemistry
Personally, I have taken my Unit 4 Chemistry in June 2017 (My stats below):
Page 1 of 67
, ReallyAcademics
Table of Contents
IAL EDEXCEL CHEMISTRY UNIT 4 ALL MULTIPLE CHOICE QUESTIONS BY TOPIC .................... 1
PREFACE ...................................................................................................................................................... 1
RATES OF CHEMICAL CHANGE ............................................................................................................. 3
ENTROPY ..................................................................................................................................................... 8
MOLAR ENTROPY OF SOLIDS, LIQUIDS AND GAS ........................................................................ 8
LATTICE ENERGY, ENTHALPY OF HYDRATION AND ENTHALPY OF SOLUTION ............... 12
CALCULATING EQUILIBRIA ................................................................................................................. 18
APPLICATION OF RATES AND EQUILIBRIUM .................................................................................. 23
ACID/BASE EQUILIBRIA ........................................................................................................................ 30
ORGANIC CHEMISTRY ........................................................................................................................... 40
ISOMERISM AND CHIRALITY ........................................................................................................... 40
ESTERS AND POLYESTERS ............................................................................................................... 42
REACTIONS OF ACYLY CHLORIDES ............................................................................................... 48
REACTIONS OF CARBONYL COMPOUND ...................................................................................... 49
ALCOHOLS ............................................................................................................................................ 52
CARBOXYLIC ACID ............................................................................................................................. 52
ORGANIC COMPOUND IDENTIDIFICATION .................................................................................. 53
SPECTROSCOPY AND CHROMATOGRAPHY ..................................................................................... 58
INFRARED SPECTRUM ....................................................................................................................... 58
MASS SPECTROSCOPY ....................................................................................................................... 59
LOW RESOLUTION AND HIGH RESOLUTION PROTON NMR SPECTRUM .............................. 60
HIGH-PERFORMANCE LIQUID CHROMATOGRAPHY.................................................................. 62
GAS CHROMATOGRAPHY ................................................................................................................. 63
OTHERS ...................................................................................................................................................... 64
NAME THE COMPOUND ..................................................................................................................... 64
POLARITY .............................................................................................................................................. 66
BOILING AND MELTING TEMPERATURES .................................................................................... 66
STRUCTURAL ISOMERISM ................................................................................................................ 67
Page 2 of 67
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RATES OF CHEMICAL CHANGE
1. In aqueous solution, iodine reacts with propanone in the presence of a catalyst of dilute hydrochloric
acid. Which of the following methods would be suitable for investigating the rate of this reaction?
(June 2014)
a. Measuring the increase in pH with a pH meter.
b. Measuring the change in rotation of plane-polarized light with a polarimeter.
c. Quenching with ice cold water, followed by titration with acid.
d. Quenching with sodium hydrogencarbonate solution, followed by titration with sodium
thiosulfate solution.
Answer
D because sodium thiosulfate will react with left over iodine after quenching reaction with sodium
hydrogencarbonate solution. The amount of iodine over time determines the rate of reaction.
A is wrong because pH will decrease instead of increase
B is wrong because there are no chiral centers
C is wrong because there is no base for it to titrate with
2. Hydrogen peroxide decomposes in a first order reaction. (June 2014)
The half-life for this reaction is 60 s.
In an experiment, the initial concentration of hydrogen peroxide is 0.100 mol dm–3.
The concentration of hydrogen peroxide, in mol dm–3, at 120 s is
a. 0.025
b. 0.050
c. 0.075
d. 0.100
Answer
A
It takes 60 seconds for 0.100 mol dm-3 to half.
At 60 seconds the concentration is 0.050 mol dm-3
At 120 seconds the concentration is 0.025 mol dm-3
3. To determine the activation energy, Ea, for a reaction, a graph was plotted of ln k against 1/T, where
k is the rate constant. (June 2014)
The Arrhenius equation is
The gradient of the graph is equal to
a. Ea
b. −Ea
c. Ea/R
d. – Ea/R
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Answer
D
y=mx+c where y is y axis value, x is x axis value, m is gradient and c is y-intercept
Substituting the values into this equation will give:
y = ln k;
m = -Ea/R;
x = 1/T;
c = constant.
4. A bromoalkane was hydrolysed by an aqueous alkaline solution. The reaction was found to be first
order with respect to the bromoalkane and zero order with respect to hydroxide ions. A bromoalkane
consistent with this information is (June 2014)
a. CH3Br
b. CH3CH2Br
c. CH3CH2CH2Br
d. (CH3)3CBr
Answer
D
Because of the bulky alkyl groups surrounding the central carbon attached to the halogen atom, there
is very little space for the nucleophile to attack. This is called steric hindrance. Because of this, the
weak carbon-halide bond must first be broken without any other molecular interefence and once a
carbocation is formed, the nucleophile will be able to attack the now positive carbon atom to form a
bond.
5. Which graph shows how the rate constant of a reaction, k, changes with temperature? (Jan 2017)
Answer
C
As temperature increases, k will increase exponentially
6. The equation for the reaction between bromate(V) ions and bromide ions in acid solution is (Jan
2016)
BrO3–(aq) + 5Br–(aq) + 6H+(aq) 3Br2(aq) + 3H2O(l)
The rate equation for this reaction is
rate = k[BrO3–][Br–][H+]2
When the concentrations of all of the reactants are doubled, the rate increases by a factor of
a. 2
b. 4
c. 8
d. 16
Answer
Page 4 of 67
IAL EDEXCEL CHEMISTRY UNIT 4 ALL
MULTIPLE CHOICE QUESTIONS BY TOPIC
PREFACE
There will 2 versions of Unit 4 past papers:
Sorted by Year
Sorted by Topic
I will also make a complete revision guide for A2 chemistry
Personally, I have taken my Unit 4 Chemistry in June 2017 (My stats below):
Page 1 of 67
, ReallyAcademics
Table of Contents
IAL EDEXCEL CHEMISTRY UNIT 4 ALL MULTIPLE CHOICE QUESTIONS BY TOPIC .................... 1
PREFACE ...................................................................................................................................................... 1
RATES OF CHEMICAL CHANGE ............................................................................................................. 3
ENTROPY ..................................................................................................................................................... 8
MOLAR ENTROPY OF SOLIDS, LIQUIDS AND GAS ........................................................................ 8
LATTICE ENERGY, ENTHALPY OF HYDRATION AND ENTHALPY OF SOLUTION ............... 12
CALCULATING EQUILIBRIA ................................................................................................................. 18
APPLICATION OF RATES AND EQUILIBRIUM .................................................................................. 23
ACID/BASE EQUILIBRIA ........................................................................................................................ 30
ORGANIC CHEMISTRY ........................................................................................................................... 40
ISOMERISM AND CHIRALITY ........................................................................................................... 40
ESTERS AND POLYESTERS ............................................................................................................... 42
REACTIONS OF ACYLY CHLORIDES ............................................................................................... 48
REACTIONS OF CARBONYL COMPOUND ...................................................................................... 49
ALCOHOLS ............................................................................................................................................ 52
CARBOXYLIC ACID ............................................................................................................................. 52
ORGANIC COMPOUND IDENTIDIFICATION .................................................................................. 53
SPECTROSCOPY AND CHROMATOGRAPHY ..................................................................................... 58
INFRARED SPECTRUM ....................................................................................................................... 58
MASS SPECTROSCOPY ....................................................................................................................... 59
LOW RESOLUTION AND HIGH RESOLUTION PROTON NMR SPECTRUM .............................. 60
HIGH-PERFORMANCE LIQUID CHROMATOGRAPHY.................................................................. 62
GAS CHROMATOGRAPHY ................................................................................................................. 63
OTHERS ...................................................................................................................................................... 64
NAME THE COMPOUND ..................................................................................................................... 64
POLARITY .............................................................................................................................................. 66
BOILING AND MELTING TEMPERATURES .................................................................................... 66
STRUCTURAL ISOMERISM ................................................................................................................ 67
Page 2 of 67
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RATES OF CHEMICAL CHANGE
1. In aqueous solution, iodine reacts with propanone in the presence of a catalyst of dilute hydrochloric
acid. Which of the following methods would be suitable for investigating the rate of this reaction?
(June 2014)
a. Measuring the increase in pH with a pH meter.
b. Measuring the change in rotation of plane-polarized light with a polarimeter.
c. Quenching with ice cold water, followed by titration with acid.
d. Quenching with sodium hydrogencarbonate solution, followed by titration with sodium
thiosulfate solution.
Answer
D because sodium thiosulfate will react with left over iodine after quenching reaction with sodium
hydrogencarbonate solution. The amount of iodine over time determines the rate of reaction.
A is wrong because pH will decrease instead of increase
B is wrong because there are no chiral centers
C is wrong because there is no base for it to titrate with
2. Hydrogen peroxide decomposes in a first order reaction. (June 2014)
The half-life for this reaction is 60 s.
In an experiment, the initial concentration of hydrogen peroxide is 0.100 mol dm–3.
The concentration of hydrogen peroxide, in mol dm–3, at 120 s is
a. 0.025
b. 0.050
c. 0.075
d. 0.100
Answer
A
It takes 60 seconds for 0.100 mol dm-3 to half.
At 60 seconds the concentration is 0.050 mol dm-3
At 120 seconds the concentration is 0.025 mol dm-3
3. To determine the activation energy, Ea, for a reaction, a graph was plotted of ln k against 1/T, where
k is the rate constant. (June 2014)
The Arrhenius equation is
The gradient of the graph is equal to
a. Ea
b. −Ea
c. Ea/R
d. – Ea/R
Page 3 of 67
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Answer
D
y=mx+c where y is y axis value, x is x axis value, m is gradient and c is y-intercept
Substituting the values into this equation will give:
y = ln k;
m = -Ea/R;
x = 1/T;
c = constant.
4. A bromoalkane was hydrolysed by an aqueous alkaline solution. The reaction was found to be first
order with respect to the bromoalkane and zero order with respect to hydroxide ions. A bromoalkane
consistent with this information is (June 2014)
a. CH3Br
b. CH3CH2Br
c. CH3CH2CH2Br
d. (CH3)3CBr
Answer
D
Because of the bulky alkyl groups surrounding the central carbon attached to the halogen atom, there
is very little space for the nucleophile to attack. This is called steric hindrance. Because of this, the
weak carbon-halide bond must first be broken without any other molecular interefence and once a
carbocation is formed, the nucleophile will be able to attack the now positive carbon atom to form a
bond.
5. Which graph shows how the rate constant of a reaction, k, changes with temperature? (Jan 2017)
Answer
C
As temperature increases, k will increase exponentially
6. The equation for the reaction between bromate(V) ions and bromide ions in acid solution is (Jan
2016)
BrO3–(aq) + 5Br–(aq) + 6H+(aq) 3Br2(aq) + 3H2O(l)
The rate equation for this reaction is
rate = k[BrO3–][Br–][H+]2
When the concentrations of all of the reactants are doubled, the rate increases by a factor of
a. 2
b. 4
c. 8
d. 16
Answer
Page 4 of 67
