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WorksheetsCCC Multiple Choice Practice. 50 questions!!
Total questions: 28
Worksheet time: 56mins
When 6 M hydrochloric acid is added to an unknown
white solid, a colorless gas is produced. What is a
possible identity for this solid?
calcium nitrate
copper (II) chloride
potassium sulfate
sodium carbonate
What is the first change that occurs when I2(s) is heated
slowly at one atmosphere pressure?
The solid melts
The solid vaporizes
The solid breaks into atoms
The solid becomes darker in colour
Two pure organic compounds melt at 112 °C and 114 °C,
respectively. If equal quantities of them are mixed, at
what temperature will the mixture begin to melt?
below 112 °C
at 112 °C
between 112 °C and 114 °C
above 114 °C
What is the major reason for using mercury (rather than
water) in barometers?
Mercury is much denser than water.
Mercury has a higher boiling point than water.
Mercury is chemically unreactive compared with
water.
Mercury expands with a decrease in air pressure;
water does not.
How can 0.1 g samples of the two white solids, lead(II)
chloride and silver chloride, be distinguished from one
another?
Add 10 mL of cold water to each. The silver
chloride will dissolve.
Add 10 mL of hot water to each. The lead(II)
chloride will dissolve.
Add 10 mL of sodium chloride to each solution. The
lead(II) chloride will become warm and release
chlorine gas.
Add 10 mL of zinc chloride solution to each. The
silver chloride will change to metallic silver.
Which is the proper way to heat a liquid in a test tube?
What is the mass of one molecule of water in grams?
3.0 × 10-23
1.7 × 10-24
1.1 × 10-21
18
If nitrogen atoms are represented as filled circles and and oxygen atoms as open circles, how much NO2 can be prepared from the mixture shown?
4 molecules
5 molecules
8 molecules
6 molecules
A mineral containing iron(II) sulfide but no other
sulfides is treated with excess hydrochloric acid to
produce hydrogen sulfide. If a 3.15 g sample of the
mineral yields 448 mL of hydrogen sulfide gas
(measured at 0 °C and 760 mm Hg), what is the mass
percentage of iron(II) sulfide in the sample?
71.0
55.8
35.5
20.4
Naturally occurring thallium consists of two stable
isotopes, Tl-203 and Tl-205 (atomic masses = 203.0 and
205.0, respectively) and has an average atomic mass of
204.4. What is the percentage of Tl-205?
14.0%
30.0%
50.0 %
70.0 %
What is the maximum mass (in grams) of NO that could be obtained from 15.5 g of N2O4 and 4.68 g of N2H4 when they react? The balanced chemical equation is;
2N2O4 + N2H4 → 6NO + 2H2O
4.38
5.04
15.2
26.2
What volume of 0.108 M H2SO4 is required to neutralize 25.0 mL of 0.145 M KOH?
16.8 mL
37.2 mL
67.1 mL
33.6 mL
A gas mixture at 27°C and 760 mm Hg contains 1.0 g
each of He, H2, N2 and CO2. How do their average
molecular speeds compare?
(A) (B)
(C) (D)
He < H2 < N2 < CO2
CO2 < N2 < He < H2
CO2 < H2 = N2 < He
He = H2 = N2 = CO2
A 2.00 liter evacuated container has a mass of 1050.0 g.
When the container is filled with an unknown gas at 800.
mm Hg pressure and 25.0 °C the mass is 1052.4 g. What
is the molar mass of the gas (in g·mol-1)?
28
31
54
56
A mixture of 0.100 mol of N2 and 0.200 mol of O2 is collected over H2O at an atmospheric pressure of 750.
mm Hg and a temperature of 22 °C. What is the partial
pressure (in mmHg) of O2 in this mixture?
478
485
500
515
A solid is insoluble in water, does not conduct
electricity, and does not melt below 1000 °C. This solid
could be
Pt.
SiC
CsCl
C10H22
Which property(ies) of a liquid increases when the temperature is raised?
I. vapor pressure
II. surface tension
I only
II only
Both I and II
Neither I nor II
Which statement is correct about the substance represented by this phase diagram?
The solid sublimes at 1 atm pressure.
The density of the solid is greater than that of the
liquid.
It exists as a liquid at 25 °C and 1 atm pressure.
Its normal boiling point is above 300K.
Which equation represents the reaction for the standard
enthalpy of formation, ΔHf°, for B5H9(g) at 298 K and 1
atm?
C2H6(g) + 7/2O2(g)→ 2CO2(g) + 3H2O(g) ΔH° = –1427.7 kJ
If the enthalpy of vaporization for H2O(l) is 44.0 kJ/mol,
what is ΔH° for this reaction if H2O(l) is formed instead
of H2O(g)?
–1559.7 kJ
–1471.7 kJ
–1295.7 kJ
–1383.7 kJ
A gold ring that weighs 3.81 g is heated to 84.0 °C and placed in 50.0 g of H2O at 22.1 °C. What is the final temperature?
53.1 °C
26.5 °
24.0 °C
22.2 °C
Calculate the change in enthalpy, ΔH, for the combustion of 11.2 L of hydrogen gas, measured at 0 °C and 1 atm pressure, to form H2O(g).
–60.5 kJ
–121 kJ
–484 kJ
–2710 kJ
Which reaction proceeds with the greatest increase in
entropy?
Br2(l) + F2(g) → 2BrF(g)
H2(g) + O2(g) → H2O2(l)
4NH3(g) + 7O2(g) → 4NO2(g) + 6H2O(g)
Cu2+(aq) + Zn(s) → Cu(s) + Zn2+(aq)
For the reaction,
N2H4(l) → N2(g) + 2H2(g) ΔH° = -50.6 kJ.
This reaction is
spontaneous only at high temperatures.
spontaneous only at low temperatures.
non-spontaneous at all temperatures.
spontaneous at all temperatures.
All of the following are expected to affect the rate of an
irreversible chemical reaction EXCEPT
adding a catalyst.
increasing the temperature.
removing some products.
decreasing the reactant concentration.
The oxidation of ammonia produces nitrogen and water
according to the equation:
4NH3(g) + 3O2(g) → 2N2(g) + 6H2O(g)
If the rate of formation of N2 at a certain temperature is
3.0 mol.L-1.s-1, what is the rate of disappearance of O2?
9.0 mol⋅L-1.s-1
4.5 mol⋅L-1.s-1
2.0 mol⋅L-1.s-1
3.0 mol⋅L-1.s-1
What are the units of the rate constant for a second order
reaction when the rate is expressed in mol.L-1 .s-1 ?
s-1
L⋅mol-1
L2⋅mol-2.s-1
L.mol-1 ⋅s-1
For the reaction:
(CH3)3CBr(aq) + OH–(aq) → (CH3)3COH(aq) + Br–(aq)
it is found that halving the concentration of (CH3)3CBr
causes the reaction rate to be halved but halving the
concentration of OH– has no effect on the rate. What is
the rate law?
