WorksheetsIndustrial Chemistry
Total questions: 60
Worksheet time: 2hrs 33mins
Name
Class
Date
1.
In vulcanised rubber, the polymer chains …
a)
are highly branched.
b)
are formed by condensation polymerisation.
c)
are unreactive.
d)
are cross-linked by sulfur atoms.
2.
One advantage of the synthetic rubber formed from styrene and butadiene over natural rubber is that …
a)
it is able to be formed by condensation polymerisation.
b)
t deteriorates more slowly.
c)
it is not derived from petrochemicals.
d)
it does not need vulcanising.
3.
Consider the system below.
2HI(g) > H2(g) + I2(g)
Which action would not cause a shift in this system?
2HI(g) > H2(g) + I2(g)
Which action would not cause a shift in this system?
a)
Increasing the temperature.
b)
Increasing the concentration of H2 only.
c)
Increasing the concentration of HI only.
d)
Increasing the volume of the flask.
4.
Consider the equilibrium system below.
Cr2O72−(aq) + H2O(l) > 2CrO42−(aq) + 2H+(aq)
Cr2O72− is orange. CrO42−(aq) is yellow. In a system that is initially a yellow-orange colour, what change will occur if a small quantity of 5M NaOH solution is added at constant temperature?
Cr2O72−(aq) + H2O(l) > 2CrO42−(aq) + 2H+(aq)
Cr2O72− is orange. CrO42−(aq) is yellow. In a system that is initially a yellow-orange colour, what change will occur if a small quantity of 5M NaOH solution is added at constant temperature?
a)
The solution will turn yellow.
b)
The concentration of H+ will increase.
c)
The concentration of Cr2O72− will increase.
d)
The value of K will change.
5.
Consider the equilibrium system below, contained in a 1.0L flask.
PCl5(g) PCl3(g) + Cl2(g)
What change will occur, relative to the initial state of the system, when the volume of the flask is increased to 3.0L at constant temperature?
PCl5(g) PCl3(g) + Cl2(g)
What change will occur, relative to the initial state of the system, when the volume of the flask is increased to 3.0L at constant temperature?
a)
Shift to the right.
b)
Pressure increases.
c)
[Cl2] increases.
d)
The value of K increases.
6.
Consider the equilibrium system below.
N2(g) + O2(g) 2NO(g)ΔH = +180kJmol−1
Which of the following will occur when the temperature is decreased in a fixed volume flask?
N2(g) + O2(g) 2NO(g)ΔH = +180kJmol−1
Which of the following will occur when the temperature is decreased in a fixed volume flask?
a)
[O2] decreases.
b)
[NO] increases.
c)
[N2] increases.
d)
Pressure increases.
7.
If a catalyst is added to a closed system not yet at equilibrium, what will occur?
a)
Equilibrium will be reached more quickly.
b)
The catalyst increases the rate of the back reaction only.
c)
No effect.
d)
The system will never reach equilibrium.
8.
Consider the system below.
N2O4(g) 2NO2(g)
What is the value of K if, at equilibrium, there is 0.600mol of N2O4 and 0.0500mol of NO2 present in a 2.00L flask?
N2O4(g) 2NO2(g)
What is the value of K if, at equilibrium, there is 0.600mol of N2O4 and 0.0500mol of NO2 present in a 2.00L flask?
a)
240
b)
0.00208
c)
480
d)
0.417
9.
Consider the system below.
2NO(g) + O2(g) 2NO2(g)
A mixture at 1000K contains 0.08M O2, 0.05M NO and 0.01M NO2. K = 0.5. Which of the following statements is true?
2NO(g) + O2(g) 2NO2(g)
A mixture at 1000K contains 0.08M O2, 0.05M NO and 0.01M NO2. K = 0.5. Which of the following statements is true?
a)
An increase in [O2] will increase K.
b)
A decrease in pressure would increase K.
c)
The system is at equilibrium.
d)
The system lies to the right.
10.
The reaction below has an equilibrium constant of 0.5 at 400°C.
N2(g) + 3H2(g) > 2NH3(g)
What would K be equal to for the following reaction at the same temperature?
NH3(g) > N2(g) + H2(g)
N2(g) + 3H2(g) > 2NH3(g)
What would K be equal to for the following reaction at the same temperature?
NH3(g) > N2(g) + H2(g)
a)
0.25
b)
1.4
c)
2.0
d)
4.0
11.
What does a very large value of K indicate?
a)
The equilibrium lies to the right.
b)
A catalyst is present.
c)
There will be no products present at equilibrium.
d)
The forward reaction has a large EA.
12.
At 700 K, the reaction below has K = 4.3 x 106.
2SO2(g) + O2(g) 2SO3(g)
In one system, the following concentrations are present:
[SO2] = 0.10M [SO3] = 10M [O2] = 0.10M
Which statement is true?
2SO2(g) + O2(g) 2SO3(g)
In one system, the following concentrations are present:
[SO2] = 0.10M [SO3] = 10M [O2] = 0.10M
Which statement is true?
a)
This system will shift to the right to reach equilibrium.
b)
The system will never reach equilibrium.
c)
This system will shift to the left to reach equilibrium
d)
This system is at equilibrium.
13.
Take a look at the equilibrium below.
2IBr(g) >I2(g) + Br2(g),
If 0.025mol of IBr is placed in a 2.00L container, and 0.0050mol is left at equilibrium, what is the value of K?
2IBr(g) >I2(g) + Br2(g),
If 0.025mol of IBr is placed in a 2.00L container, and 0.0050mol is left at equilibrium, what is the value of K?
a)
3.0
b)
4.0
c)
2.0
d)
1.0
14.
Methanol is produced commercially by the acid–catalysed reaction of carbon monoxide and hydrogen. Both reactants and products are gaseous. An equilibrium mixture in a 2.00L container was found to contain 0.0406mol of methanol, 0.170mol of carbon monoxide, and 0.302mol of hydrogen at 500K. What is the value of K?
a)
0.0952
b)
2.62
c)
0.382
d)
10.5
15.
What is the major use of sulfuric acid?
a)
Petroleum refining.
b)
Manufacturing explosives.
c)
Manufacturing superphosphate fertiliser.
d)
Manufacturing ammonium sulfate fertiliser.
16.
Sulfuric acid is used as the electrolyte in which battery?
a)
Leclanché cell.
b)
Alkaline cell.
c)
Lead-acid.
d)
Fuel cell.
17.
What is the name of the process used to extract sulfur from underground deposits?
a)
Distillation
b)
Electrolysis
c)
Frasch process
d)
Membrane process
18.
The name of the process used to manufacture most sulfuric acid is the …
a)
contact process
b)
Frasch process
c)
lead chamber process
d)
esterification
19.
The second step in the production of sulfuric acid is:
2SO2(g) + O2(g) > 2SO3(g) + heat
Which conditions would increase the rate of this reaction?
2SO2(g) + O2(g) > 2SO3(g) + heat
Which conditions would increase the rate of this reaction?
a)
Catalyst, high temperature, high pressure.
b)
Catalyst, high temperature, low pressure.
c)
Catalyst, low temperature, low pressure.
d)
Catalyst, low temperature, high pressure.
20.
The second step in the production of sulfuric acid is
2SO2(g) + O2(g) > 2SO3(g) + heat
Which conditions would increase the yield of this reaction?
2SO2(g) + O2(g) > 2SO3(g) + heat
Which conditions would increase the yield of this reaction?
a)
High temperature, high pressure.
b)
Low temperature, high pressure.
c)
High temperature, low pressure.
d)
Low temperature, low pressure.
21.
Which catalyst is used in the contact process?
a)
H2SO4
b)
MnO2
c)
V2O5
d)
Pt
22.
What is the formula of oleum?
a)
H2S2O7
b)
H2SO4
c)
H2SO3
d)
H2S
23.
Which problem could not be caused by sulfur dioxide emissions?
a)
Acid rain.
b)
Respiratory disease.
c)
Crop damage.
d)
Photochemical smog
24.
What are the products of the reaction between sucrose and concentrated sulfuric acid?
a)
Carbon dioxide and water.
b)
Carbon and water.
c)
Carbon, hydrogen and oxygen gas.
d)
Carbon monoxide and hydrogen.
25.
What are three conditions that exist in the converter to maximise the conversion of SO2 to SO3?
a)
Several catalyst beds, heat retained, excess oxygen used.
b)
Several catalyst beds, heat retained, excess oxygen used.
c)
One catalyst bed, excess heat removed, excess sulfur dioxide used.
d)
Several catalyst beds, excess heat removed, excess oxygen used.
26.
Great care must be taken when diluting concentrated sulfuric acid because …
a)
sulfuric acid is caustic.
b)
sulfuric acid is expensive.
c)
the reaction is highly exothermic.
d)
the reaction has a slow rate.
27.
Which statement is true for both galvanic and electrolytic cells?
a)
The anode has a positive polarity.
b)
Electrodes are immersed in the same electrolyte.
c)
The anode is the site of oxidation.
d)
A power source is needed.
28.
Which statement is true for galvanic cells but not electrolytic cells?
a)
The cathode is positive.
b)
The emf can be negative.
c)
Electrons travel from anode to cathode.
d)
The anode is the site of oxidation.
29.
Two graphite rods are inserted into molten zinc chloride and connected to a power source as pictured.
Which statement is false in regard to this cell?
Which statement is false in regard to this cell?
a)
Chloride ions are oxidised.
b)
No salt bridge is needed.
c)
Zinc ions are reduced.
d)
Electrons travel from cathode to anode.
30.
Two graphite electrodes are inserted into an aqueous solution of nickel(II) iodide and connected to a power source.
In this cell …
In this cell …
a)
water is oxidised.
b)
electrons travel from the cathode to the anode.
c)
Ni2+ ions migrate to the anode.
d)
Ni2+ is reduced.
31.
Which of the following reduction reactions has the greatest tendency to proceed as written?
a)
Cd2+(aq) + 2e− Cd(s) E° = −0.40V
b)
2H+(aq) + 2e− H2(g) E° = 0.00V
c)
Hg2+(aq) + 2e− Hg(l) E° = +0.85V
d)
Au3+(aq) + 3e− Au(s) E° = +1.50V
32.
Which of these substances will not be produced by the electrolysis of concentrated sodium chloride solution (brine)?
a)
Hydrogen
b)
Chlorine
c)
Hydroxide ions
d)
Oxygen
33.
The predominant product at the anode in a chlor-alkali cell is …
a)
Hydrogen
b)
Chlorine
c)
Hydroxide ions
d)
Oxygen
34.
The major disadvantage of the diaphragm process is that …
a)
it is very costly.
b)
it uses asbestos.
c)
it uses mercury.
d)
it produces diluted sodium hydroxide.
35.
A major advantage of the membrane process is that …
a)
the sodium hydroxide produced has high purity.
b)
it is inexpensive.
c)
it produces less chlorine.
d)
it produces less chlorine. it doesn't use as much brine.
36.
The cathode in the mercury process consists of …
a)
Graphite
b)
Titanium
c)
Iron
d)
Mercury
37.
In regard to the membrane process, which statement is false?
a)
The cathode is made of steel.
b)
The anode is made of titanium.
c)
Both compartments have brine flowing into them.
d)
Chlorine is produced at the anode.
38.
The molecular formula of glycerol is …
a)
C2H6O2
b)
C4H10O4
c)
C3H8O3
d)
CH3OH
39.
Which of the following is a soap?
a)
CH3COONa
b)
C18H37COONa
c)
C3H8O3
d)
C17H35C6H4SO3Na
40.
Lye is used in soap-making. Lye is a concentrated solution of which ionic compound?
a)
CuSO4
b)
NaCl
c)
K2CO3
d)
NaOH
41.
What type of bond would exist between this soap and oil?
a)
Dispersion forces
b)
Hydrogen bonds
c)
Covalent bonds
d)
Dipole-dipole forces
42.
A good surfactant will have a …
a)
hydrophilic head and a short hydrophobic tail.
b)
hydrophobic head and tail.
c)
hydrophilic head and tail.
d)
hydrophilic head and a long hydrophobic tail.
43.
Which of the following occurs when a greasy plate is placed in soapy water and scrubbed?
a)
The hydrophobic tail of the soap bonds to water.
b)
The soap froths but does not actually bond with the grease.
c)
The hydrophilic head of the soap bonds to grease.
d)
The hydrophobic tail of the soap bonds to grease.
44.
Hydrophobic is another name for a substance which …
a)
attracts water.
b)
repels oil.
c)
bonds weakly to water.
d)
bonds weakly to oil.
45.
When oil and water are poured into the same vessel, two layers are observed with the less dense oil on top. These two liquids are said to be …
a)
hydrophobic.
b)
insoluble.
c)
hydrophilic.
d)
immiscible.
46.
Which of the following is not an essential part of an emulsion?
a)
Emulsifier.
b)
Oil.
c)
Water.
d)
Dissolved salt.
47.
Soaps cannot be used in hard water because they …
a)
form precipitates.
b)
create environmental problems.
c)
are too greasy.
d)
contain sodium.
48.
When sodium stearate, CH3(CH2)16COONa, is added to hard water, the formula of one possible precipitate is …
a)
(CH3(CH2)16COO)2Ba
b)
(CH3(CH2)16COO)2Cd
c)
(CH3(CH2)16COO)2Ca
d)
CH3(CH2)16COOK
49.
The species pictured is …
a)
an anionic surfactant.
b)
a soap.
c)
a cationic surfactant.
d)
a non-ionic surfactant.
50.
An advantage of detergents over soaps is …
a)
detergents always contain anionic heads.
b)
detergents are cheaper to make.
c)
detergents are biodegradable.
d)
detergents do not precipitate in hard water.
51.
Which of the following would be an appropriate use of a non-ionic detergent?
a)
Powder for front-loading washing machines.
b)
Liquid hand soap.
c)
Toothpaste
d)
Glass cleaners.
52.
Detergents with branched hydrocarbon chains are less likely to be …
a)
sulfonates.
b)
effective.
c)
biodegradable.
d)
synthetic.
53.
Another name for sodium carbonate is …
a)
Caustic soda
b)
Soda ash
c)
Lye
d)
Washing soda
54.
What is currently the major use of sodium carbonate?
a)
Glass-making.
b)
Ink removal from paper.
c)
Water-softening.
d)
Soap-making.
55.
Calcium carbonate is also known as …
a)
limestone.
b)
soda ash.
c)
washing soda.
d)
lime.
56.
What is the overall equation for the Solvay process?
a)
NH3(aq) + CO2(aq) + NaCl(aq) + H2O(l) NaHCO3(aq) + NH4Cl(aq)
b)
CaO(s) + H2O(l) Ca(OH)2(aq)
c)
CaCO3(s) + 2NaCl(aq) Na2CO3(s) + CaCl2(aq)
d)
CaCO3(s) CaO(s) + CO2(g)
57.
How is brine purified before being used in the Solvay process?
a)
Fractional crystallisation.
b)
Centrifuging.
c)
Distillation.
d)
Filtration.
58.
At 0°C sodium hydrogencarbonate is easily separated from ammonium chloride in solution because of their difference in …
a)
boiling point.
b)
solubility.
c)
density.
d)
reactivity.
59.
How is sodium hydrogencarbonate converted to sodium carbonate?
a)
Dissolution
b)
Heating
c)
Distillation
d)
Filtration
60.
Which substance is not recycled during the Solvay process?
a)
CO2
b)
H2O
c)
Cl−
d)
NH3
100 %
