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WorksheetsChemistry HSC Quiz mixed
Total questions: 40
Worksheet time: 1hrs 27mins
Name
Class
Date
1.
When bromine (Br2) reacts with ethylene (C2H4), what type of reaction occurs?
a)
Addition (hydration).
b)
Addition (hydrohalogenation).
c)
Addition (halogenation).
d)
Addition (hydrogenation).
2.
Which statement is true of addition polymerisation but not condensation polymerisation?
a)
Many monomers link together to form polymers.
b)
Only one type of monomer is used.
c)
An organism is needed for the synthesis reaction.
d)
Only one product is formed.
3.
When a polyester forms, the two functional groups that react to form the ester link between the monomers are …
a)
–OH and –COOH.
b)
–NH2 and –COOH.
c)
–NH2 and –OH.
d)
–OH and –OH.
4.
What is the molecular formula of the monomer used to make this polymer (polyvinylidene chloride)?
a)
C2H3Cl
b)
C2HCl3
c)
C4H4Cl4
d)
C2H2Cl2
5.
Which of these equations correctly represents the fermentation of glucose catalysed by yeast in anaerobic conditions?
a)
C12H22O11(aq) + 12O2(g) >12CO2(g) + 11H2O(l)
b)
C6H12O6(aq) + 6O2(g) > 6CO2(g) + 6H2O(l)
c)
C6H12O6(aq) > 2C2H5OH(aq) + 2CO2(g)
d)
C12H22O11(aq) + H2O(l) > 4C2H5OH(aq) + 4CO2(g)
6.
Ethanol has a similar molecular mass to propane and yet ethanol's boiling point is 120°C higher. The best explanation for this is that …
a)
the dipole-dipole forces present between propane molecules are not as strong as those between ethanol molecules.
b)
the dispersion forces present between ethanol molecules are stronger than those between propane molecules.
c)
propane molecules exert a repulsive effect on each other.
d)
ethanol molecules are able to hydrogen bond with each other.
7.
In a calorimetry experiment, 150mL of water was heated by 0.350g of octane. During this time, the temperature of the water increased from 20.0°C to 46.7°C. What is ΔHc of octane?
a)
-2736kJmol−1
b)
–10942kJmol−1
c)
–3647kJmol−1
d)
–5471kJmol−1
8.
Dynamic equilibrium can best be described as …
a)
an open system in which all reactions have ceased.
b)
a closed system in which the rate of the forward reaction equals the rate of the back reaction.
c)
an open system in which the rate of the forward reaction equals the rate of the back reaction.
d)
closed system in which all reactions have ceased.
9.
The graph below shows that …
a)
at the start of the reaction, only NO2 was present.
b)
the system never reaches equilibrium.
c)
more NO2 is present at equilibrium than N2O4.
d)
the rate of reaction slowly increases.
10.
Le Chatelier's principle states that, 'If a chemical system at equilibrium is subjected to a change in conditions, the system will ….'
a)
react in a way that neutralises the change incurred
b)
not respond in any way
c)
react in a way that quickly returns all reactant and product concentrations to their original values
d)
adjust to re-establish equilibrium in such a way as to partially counteract the imposed change
11.
What change occurred to the system at t = 5 minutes?
a)
Pressure increased.
b)
NO2 added.
c)
Volume decreased.
d)
Temperature decreased.
12.
Consider the equilibrium system below.N2(g) + O2(g) > 2NO(g)What change would occur if the volume of the system was halved at constant temperature?
a)
Concentrations halved, no shift.
b)
Concentrations double, shift to the right.
c)
Concentrations halved, shift to the left.
d)
Concentrations double, no shift.
13.
The forward reaction of the following equilibrium system is exothermic.N2(g) + 3H2(g) > 2NH3(g)How would a 30°C increase in temperature affect this system?
a)
Reaction rates increase, shift to the left.
b)
Reaction rates decrease, shift to the right.
c)
Reaction rates increase, shift to the right.
d)
Reaction rates decrease, shift to the left.
14.
Which acid would not have been classed as acidic by Lavoisier?
a)
HNO3
b)
HCl
c)
CH3COOH
d)
H2SO4
15.
Humphry Davy proposed that all acids …
a)
are proton donors.
b)
contain oxygen.
c)
contain hydrogen.
d)
produce hydrogen ions in solution.
16.
Arrhenius defined an acidic substance as one which …
a)
is an electron pair acceptor.
b)
is a proton donor.
c)
contains oxygen.
d)
produces hydrogen ions in water.
17.
What number of moles of hydrochloric acid is needed to react with 0.10 moles of aluminium hydroxide?
a)
0.10 moles.
b)
0.20 moles.
c)
0.40 moles.
d)
0.30 moles.
18.
NH4+ is best described as …
a)
a strong acid.
b)
a strong base.
c)
a weak acid.
d)
a weak base.
19.
Which of the following species is not amphiprotic?
a)
H2O
b)
HCO3−
c)
CO32−
d)
H2PO4−
20.
Which of the following is not a conjugate acid-base pair?
a)
HCl/Cl−
b)
HCO3−/CO32−
c)
HNO3/NO3−
d)
H2SO4/SO42−
21.
Pure gastric juice in the stomach has a pH of approximately 1. How many times more acidic is this than pure water?
a)
10 000
b)
100
c)
1 000 000
d)
10 000 000
22.
HCl is a strong acid, while CH3COOH is a weak acid. Which of the following statements would be true of 0.1 M solutions of both species?
a)
The pH of the HCl solution would be higher than the pH of the CH3COOH solution.
b)
The pH of the HCl solution would be lower than the pH of the CH3COOH solution.
c)
There will be a lower concentration of H3O+ ions in the HCl solution.
d)
The pH of both solutions would be equal to 1.
23.
Phenolphthalein is an indicator that turns from colourless to pink over pH 8.2. A 0.001M solution of which species would be most likely to turn phenolphthalein pink?
a)
NaHSO4
b)
NaOH
c)
CH3OH
d)
NH3
24.
An aqueous solution has a pH of 4.0. What is the concentration of hydroxide ions in this solution?
a)
1.0 × 10−11M
b)
10M
c)
4.0M
d)
1.0 × 10−3M
25.
Which of these equations best represents the self-ionisation of pure water?
a)
2H2O(l) <> H3O+(aq) + OH−(aq)
b)
2H2O(l) <> 2H2(g) + O2(g)
c)
H+(aq) + H2O(l) <> H3O+(aq)
d)
OH−(aq) + H+(aq) <> H2O(l)
26.
A buffer solution …
a)
is never found in natural systems.
b)
has pH > 10.
c)
is able to resist small changes in pH.
d)
always contains ethanoic acid.
27.
The buffer system that controls the pH of blood is …
a)
H2CO3(aq) + H2O(l) <> H3O+(aq) + HCO3−(aq)
b)
NH4+(aq) + H2O(l) <> H3O+(aq) + NH3(aq)
c)
H2PO4−(aq) + H2O(l) <> H3O+(aq) + HPO42−(aq)
d)
CH3COOH(aq) + H2O(l) <> H3O+(aq) + CH3COO−(aq)
28.
A 0.3050M solution of HCl was titrated against 25.00mL of NaOH solution. If 18.65mL of HCl was required to reach the end point, what is the concentration of the NaOH solution?
a)
0.4088M
b)
0.2275M
c)
2.275 × 10−4M
d)
0.3050M
29.
At approximately what pH will the equivalence point occur for the titration between HCl(aq) and NaOH(aq)?
a)
4
b)
7
c)
8
d)
0
30.
Which indicator would be appropriate for the titration of 0.100M HCl with approximately 0.1M NH3?
a)
Methyl orange.
b)
Phenolphthalein.
c)
Litmus.
d)
Bromothymol blue.
31.
What is the name of the catalyst used in esterification reactions?
a)
Vanadium(V) oxide.
b)
Sulfuric acid.
c)
Cobalt(II).
d)
Platinum.
32.
The major organic product of the esterification reaction between ethanol and butanoic acid is …
a)
ethyl butanoate.
b)
propyl propanoate.
c)
water.
d)
butyl ethanoate.
33.
In many countries, fish with more than 0.500ppm mercury is considered unsafe. In one experiment, a 0.750g piece of tuna was appropriately treated and made up to 10.0mL solution. This solution returned an absorbance of 0.70. Using the calibration graph below, what can be concluded from this analysis?
a)
The concentration of mercury is exactly equal to 0.500ppm and may or may not be safe to eat.
b)
The concentration of mercury in the tuna is less than 0.500ppm and it can be eaten safely.
c)
The tuna does not contain mercury.
d)
The concentration of mercury in the tuna is greater than 0.500ppm and it should not be eaten
34.
The ion that gives a green colour in a flame test and forms a blue precipitate with OH− is …
a)
Ba2+.
b)
Cu2+.
c)
Fe2+.
d)
Ca2+.
35.
Which anion gives no precipitate with AgNO3solution but gives a white precipitate with BaCl2solution which is insoluble in HNO3 solution?
a)
Cl−
b)
CO32−
c)
PO43−
d)
SO42−
36.
In a gravimetric analysis experiment to determine the sulfate content of Happy Grow Fertiliser, 1.00g of fertiliser yielded 1.56g of dry barium sulfate precipitate. What is the percentage by mass of sulfate in this fertiliser?
a)
42.9%
b)
0.824%
c)
10.3%
d)
64.1%
37.
What is the correct equation for the Haber process?
a)
N2(g) + 3H2(g) <> 2NH3(g)
b)
N(g) + 3H(g) <> NH3(g)
c)
N2(g) + 4H2(g) <> 2NH4+(g) + 2e−
d)
N2(g) + 2H2(g) <> N2H4(g)
38.
What is the correct name for the alkyne shown?
a)
butyne
b)
but-1-yne
c)
but-2-yne
d)
1-methyl-1-propyne
39.
Alkenes are:
a)
saturated, because they do not have the maximum number of hydrogen atoms
b)
unsaturated, because they do not have the maximum number of hydrogen atoms
c)
unsaturated, because they have the maximum number of hydrogen atoms
d)
aromatic compounds
40.
What is the correct IUPAC name for the following compound?
a)
2-chloro-3-fluorobutane
b)
2-fluoro-3-chlorobutane
c)
3-fluoro-2-chlorobutane
d)
3-chloro-2-fluorobutane
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