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Super-Quiz QF-B
Gertz-Ressler High School
Chemistry 2
DO NOT write on the booklet
Standard 4: Gases
1. (4.a) In the following diagram, what is the
relationship observed between the variables?
5. (4.a) According to the Kinetic theory, pressure
over a wall is caused by:
a) Particles colliding against the wall
b) Gravity
c) Water vapor
d) Activation energy
6. (4.f) What is Zero absolute?
a) 32oF
b) 0oC
c) -273 K
a) Temperature increases, volume decreases
b) Volume decreases, pressure increases
c) Volume increases, temperature increases
d) None
2. (4.a) According to the Kinetic theory, if
the temperature in a gas system increases,
the gas particles will move faster. Choose the
correct statement below:
a) If the temperature increases and the
volume stays the same, the pressure
increases.
b) If the temperature increases and the
volume stays the same, the pressure
decreases.
c) If the temperature increases and the
pressure increases, the number of moles of
particles also increases.
d) If the temperature increases and the
volume increases, the pressure increases.
3. (4.e) Convert 70oC to Kelvin?
a) -70 K b) 343 K
c) 203 K
d) 373 K
4. (4.c) What is the volume of 2 moles of gas
at STP?
a) 44.8 L b) 11.2 L c) 22.4 L d) 30 L
d) 0 K
7. (4.d) What is “STP conditions”?
a) P = 1 atm, T = 0 oC
b) P = 1 atm, T = 0 oF
c) P = 0 atm, T = 0 oC
d) P = 1 atm, T = 25 oC
8. (4.i) Dalton’s Law says that the total pressure of
a mixture of gases is:
a) 1 atm
b) The sum of all the partial
pressures of the gases
c) Variable
d) None
Standard 5: Acids, Bases and Salts
9. (5.a) The correct formula for hydrofluoric acid
is:
a) HFO4
b) HF
c) H4F
d) HFO3
10. (5.a) The taste of acids is
a) sweet
b) sour
c) bitter
d) salty
11. (5.d) An acidic solution has a pH that is
a) more than 7
b) = 7
c) less than 7
d) any value
12. (5.d) A neutral solution
a) completely dissociates in water
b) partially dissociates in water
c) has a pH = 7
d) changes color
13. (5.c) A strong acid
a) partially dissociates in water
b) completely dissociates in water
c) changes color
d) has a pH = 7
19. (6.a) What is a chemical solution?
a) any mixture
b) heterogeneous mixture
c) homogeneous mixture
d) non-polar substance
14. (5.a) A neutralization reaction between
an acid and a base always produces
a) water and salt
b) water and basic anhydride
c) salt and basic anhydride
d) salt and acidic anhydride
20. (6.d) How many moles of CaCO3 are needed to
prepare 5.0 liters of a 2.0 M solution of CaCO3?
a) 5 moles
b) 10 moles
c) 20 moles
d) none
15. (5.b) Arrhenius defines an acid as a
substance that
a) donates H+
b) donates OHc) accepts H+
d) accepts OH16. (5.c) Complete the dissociation of HBr
HBr + H2O  ________ + _________
a) H2Br + HOc) HBr2- + O+
b) Br- + H3O+
d) BrO- + HO+
17. (5.a) Rolaids®, active ingredient:
Mg(OH)2, is the name of _________ used
to fight high _________ .
a) gas, indigestion
b) salt tablets, fever
c) acid tablets, alkalinity
d) base tablets, acidity
Standard 6: Chemical Solutions
18. (6.a) What is a solute?
a) any substance
b) medium that dissolves a substance
c) substance being dissolved
d) mixture of substances
21. (6.a) A saturated solution has a __________
amount of solute.
a) less than maximum
b) maximum possible
c) more than maximum
d) none
22. (6.a) What is the meaning of aqueous solution?
a) The solution is ionic
b) The solute is water
c) The solution is an electrolyte
d) The solvent is water
23. (6.b) When 1 mol of K2SO4 dissociates in
water, it produces ______ of K+ ions. (Balance
the equation first)
a) 1 mol
__ K2SO4  __ K+ + __ SO4b) 2 moles
c) 3 moles
d) 4 moles
24. (6.b) Chemists often say “like dissolves like.”
What does this statement mean?
a) A substance will dissolve always
b) Polar/Ionic solvent dissolves polar/ionic solute
c) Something dissolves like salt
d) It is likely that the solute will dissolve
25. (6.c) Generally, the rate of dissolution of a
solid in a liquid increases when the temperature
_________.
a) Increases
b) Decreases
c) Is constant
d) is Standard
26. (6.d) What is the mass % of solute in a solution
that contains 30g of solute and 30g of water?
a) 100%
b) 50%
c) 30%
d) none
Standard 7: Chemical Thermodynamics
27. (7.c) When water changes phase
from liquid to gas, the process is
a) Exothermic
b) Endothermic
c) Neutral
d) Kinetic
28. (7.c) The temperature of iced water
melting is _____ oC. The temperature of
boiling water is _____ oC.
a) 100, 200
b) 0, 100
c) 100, 0
d) None
29. (7.b) If in a chemical reaction, the
products have more potential energy than
the reactants, the reaction is…
a) Exothermic
b) Endothermic
c) Neutral
d) Kinetic
30. (7.d) A substance was tested for its
behavior when heated. It was first a solid;
then by adding energy it warmed-up and
melted, then more heat was added so it
warmed-up more and boiled. The following
graph of temperature was obtained:
32. (7.a) Temperature is the measure of …
a) The chemical bonds in a substance
b) The pressure of a gas
c) The actual size of the molecules
d) The kinetic energy of the particles in a
substance
33. (7.b) A sample ofwater changes temperature
from 56 oC to 20 oC. This process is
a) Exothermic
b) Endothermic
c) Neutral
d) Kinetic
34. (7.d) Problem. Use the same set of formulas
and constants. You want to evaporate 400.0 g of
water. Calculate the amount of heat needed. (Hv of
water = 2,256 J/g)
a) 1,128,000 J
b) 400 J
c) 902,400 J
d) 2,256 J
35. (7.d) Problem. Use the formulas and
constants below. You want to heat 400.0 g of water
from 20oC to 65 oC. Calculate the amount of heat
needed. (Cp of water = 4.18 J/goC)
a) 400.0 J
b) 75,240 J
c)
19,176 J
d) 52,250 J
135
Formulas
92
o
C
-12
-40
Energy, Joules
-40
From the graph, the liquid was warmed-up
from ______ to ______ oC.
a) -40, -12
b) -12, 92
c) 92, 135
d) -40, 92
31. (7.a) Heat flows from a _______ to a
_______ body.
a) Soft, Hard
b) Cold, Hot
c) Big, Small
d) Hot, Cold
Sensible heat:
Q = m Cp ΔT
Change of temperature:
Latent heat (evaporation):
Latent heat (evaporation):
ΔT = T2 – T1
Q= m Hv
Q= m Hf
Constants for water
Heat capacity:
Cp(water) = 4.18 J/g oC
Latent heat (vaporization):
Hv(water) = 2,256 J/g
Latent heat (fusion):
Hf(water) = 333 J/g
Std 8: Rate of Reaction
36. (Std 8) The energy required to start a reaction
is called…
a) Energy of reaction
b) Released energy
c) Energy of activation
d) Energy of catalyst
37. (Std 8) A change in concentration of
reactants or products over time is the:
a) Activated complex
b) Transition state
c) Reaction rate
d) Intermediate product
38. (Std 8) Catalysts...
a) Slow the rate of a reaction
b) Increase the energy of the reactants
c) Lower the activation energy
d) Are used up in reactions
39. (Std 8) For a reaction to take place,
the molecules need both to:
a) be acid, and base
b) be ionic, and covalent
c) collide with enough energy, and with
correct orientation
d) None of the above
40. (Std 8) For a particular reaction,
rate = k[A]2[B][C]3
If the concentration of reactant B is
doubled, the rate is increased by a factor
of:
a) 2
b) 4
c) 1/2
d) 1/4
41. (Std 8) Consider the following reaction
in the gas phase:
N2O4 (g)
2NO2
(g)
If you increase the pressure over this
system, the rate of reaction will
a) Decrease
b) Increase
c) Stop
d) Doesn’t affect
Std 9: Chemical Equilibrium
42. (Std 9) Choose the expression for k, the
equilibrium constant, for the reaction:
2NO2 (g)
N2O4 (g)
a)
[ N2O4 ]
K= ----------------[ NO2 ] 2
[ NO2 ] 2
b) K = -------------------[ N2O4 ]
c)
[ N2O4 ] 2
K= ----------------[ NO2 ]
d) K = [ NO2 ] 2 [ N2O4 ]
43. (Std 9) LeChatelier’s principle establishes
that:
a) The reactants are the same as the products
b) Equilibrium is a stress
c) A system will act in order to re-establish
equilibrium
d) The reactants are at the left side
Std 10: Organic Chemistry
44. A molecule of hexene has
a) only single bonds between carbons
b) a carbon-carbon double bond
c) a carbon-carbon triple bond
d) a hexagonally shaped ring structure
45. What functional group contains a hydrocarbon
which ends in OH?
a) alcohol
b) ketone
c) ether
d) amine
46. Which compounds have carbon-carbon double
bonds?
a) alkanes
b) alkenes
c) alcohols
d) ionic compounds
47. The simplest organic compound is
a) aspirin
b) table sugar
c) salt
d) methane
48. Polymers are large organic molecules
that are made of
a) cations
b) anions
c) carbon and oxygen only
d) repeating
units
49. Protein molecules are complex polymer
molecules made up of repetitive monomers
called
a) nitrogenous bases b) amino acids
c) simple sugars
d) vitamins
50. What is the name of a hydrocarbon
containing a 6-carbon chain?
a) pentane
b) propane
c) hexane
d) heptane
51. Alkanes are hydrocarbons that contain
a) single covalent bonds only
b) single or double covalent bonds.
c) carbon and oxygen only
d) carbon, hydrogen, and oxygen.
52. Alcohols are organic compounds that
contain
a) carbon and oxygen only
b) carbon and hydrogen only
c) carbon, oxygen, and hydrogen
d) carbon, nitrogen, and hydrogen
53. Carbon can form a large variety of
compounds from simple to highly complex
due to its ability to
a) form ions with four different charges
b) form four covalent bonds
c) share electrons with itself
d) form ionic bonds with many elements
54. The name of hydrocarbon compounds, such as
methane, contains two parts: a prefix (meth) and a
suffix (ane). The prefix tells
a) the number of hydrogen atoms present
b) the number of carbon atoms present
c) whether single, double or triple C-C bonds are
present
d) whether the molecule is a straight-chain or a
ring
Std 11: Nuclear Chemistry
55. The decay of C-14 is used as a tool for…
a) X-Rays
b) Making fuel
c) Dating fossil samples
d) Making organic
compounds
56. Complete the following nuclear equation:
239
__
Np
___
93
a)
0
239
Th
90
b)
239
92
U
e
+
__
-1
c)
239
Pu
94
d)
238
Pu
94
57. The most abundant isotope of lead contains 82
protons and 124 neutrons packed closely together
in the nucleus. Why do the protons stay together in
the nucleus rather than fly appart?
a) Electrons in neighboring atoms neutralize
repulsive forces between protons.
b) Nuclear forces overcome repulsive forces
between protons in the nucleus.
c) Electrostatic forces between neutrons and
protons hold the nucleus together.
d) Neutrons effectively block the protons and keep
them far apart to prevent repulsion.
58. A 2 cm thick piece of cardboard
placed over a radiation source would be
most effective in protecting against which
type of radiation?
a) Alpha
b) Beta
c) Gamma
d) X-ray
59. Which of the following lists ranks
nuclear radiation from most massive to
least massive?
a) alpha, beta, and gamma
b) beta, gamma, and alpha
c) gamma, alpha, and beta
d) gamma, beta, and alpha
60. What is the half-life of an isotope if
40 g of a 320 g sample of the isotope
remains after 18.0 years?
a) 1.0 years b) 3.0 years
c) 6.0 years
d) 9.0 years
61. A big nucleus splitting into two smaller ones,
accompanied by a great emission of energy, is
a) nuclear fusion
b) nuclear fission
c) nuclear power
d) nuclear radiation
62. Complete the following nuclear equation:
238
__
U
4
2
He
U
____
+
92
a)
239
__
b)
1
0
n
c)
92
1
1
H
d)
0
-1
e
63. The time it takes for ½ of a sample of
radioactive material to decay is…
a) Average life
b) Expected life
c) Half-life
d) Decay time
***END OF TEST, STOP AND REVIEW***
QFGR2B.doc J. Bermudez