Name: __________________________ Date: _____________
CORRECT ANSWER = CHOICE A
1. Complete and balance the following redox equation using the set of smallest
whole–numbers coefficients. What is the sum of the coefficients?
HI + HNO3  I2 + NO (acidic solution)
A) 17
B) 14
C) 7
D) 5
E) 10
2. Consider the reaction
CuO(s) + H2(g)  Cu(s) + H2O(l).
In this reaction, which substances are the oxidizing agent and reducing agent,
respectively?
A) CuO and H2
B) H2 and CuO
C) CuO and Cu
D) H2O and H2
E) H2 and Cu
3. The compound CFCl3 is used as a
A) coolant.
B) CFC replacement.
C) enzyme.
D) anesthetic.
E) gaseous fuel.
4. What is the name given the condition leading to the formation of ice particles over
Antarctica?
A) polar stratospheric clouds (PSCs)
B) vortex traps (VTs)
C) polar ice caps (PICs)
D) ice deposition (ID)
E) polymorphs (PMs)
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5. In order for a gas to be a “greenhouse gas” it must
A) transmit visible light and absorb infrared radiation.
B) be radioactive.
C) transmit infrared light and absorb visible light.
D) absorb both visible light and infrared radiation.
E) absorb both visible light and ultraviolet radiation.
6. How many different ways can a CO2 molecule vibrate when absorbs electromagnetic
radiation?
A) 4
B) 3
C) 2
D) 1
E) millions
7. Which below is a HFC?
A) CF3CFH2
B) CF3CHCl2
C) C2F3Cl3
D) CF2Cl2
E) CFCl3
8. Which one of the following is not a greenhouse gas?
A) O2
B) CO
C) NO
D) NO2
E) CFCs
9. Which of the following is a tert-butyl group?
A) –C(CH3)3
B) –CHCH2C(CH3)3
C) –CH2CH2CH2CH3
D) –CH(CH3)2
E) –CH(CH3)CH2CH3
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10. The two molecules represented below are examples of
CH3CH2OCH2CH3
CH3CH2CH2CH2OH
A) structural isomers.
B) geometric isomers.
C) optical isomers.
D) stereoisomers.
E) None of these.
11. The systematic name for the compound represented below is
A)
B)
C)
D)
E)
CH2CH3
|
CH3CH2CH2CHCHCH3
|
CH2
|
CH2CH3
3-methyl-4-propylheptane
3-ethyl-4-propylhexane
3-propyl-4-ethylhexane
4,5-diethylheptane
2-ethyl-4-propylhexane
12. Organic compounds with the general formula ROR (where R is an alkyl group) are
called
A) ethers.
B) carboxylic acids.
C) aldehydes.
D) alcohols.
E) esters.
13. Which of the following is a condensation reaction?
A) linking an acid and an alcohol to make an ester and water
B) oxidation of ethanol to acetaldehyde
C) hydrolysis of an ester
D) addition of H2 to an alkene
E) addition of H2O to a double bond
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14. Polystyrene results from the polymerization of
A) C6H5–CH=CH2
B) CF2=CF2
C)
D)
E) CH3CH=CH2
15. The nitric oxide gas reacts with chlorine gas according to the equation
NO + ½ Cl2  NOCl
The following initial rates of reaction have been calculated for the given constituent
concentrations.
Expt. No.
Rate (M/h)
NO (M)
Cl2 (M)
1
0.59
0.25
0.25
2
2.39
0.50
0.25
3
4.79
0.50
0.50
Which of the following is the rate law (rate equation) for this reaction?
A) rate = k[NO]2[Cl2]
B) rate = k[NO][Cl2]½
C) rate = k[NO][Cl2]
D) rate = k[NO]
E) rate = k[NO]2[Cl2]2
16. If suppose a first–order reaction X  Y is 25% completed in 42 min at 25°C. What is
its rate constant?
A) 6.8 × 10–3 min–1
B) 8.3 × 10–3 min–1
C) 3.3 × 10–2 min–1
D) –3.3 × 10–2 min–1
E) 11 min–1
17. Which of the following is the correct unit for a second–order rate constant?
A) M–1s–1
B) M–2s–1
C) Ms
D) Ms–1
E) s–1
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18. The nitrogen dioxide decomposes according to the reaction
2NO2(g)
2NO(g) + O2(g)
–13
while Kp = 4.48 × 10 at 25°C. What is the value for Kc?
A) 1.83 × 10–14
B) 1.81 × 10–16
C) 4.48 × 10–13
D) 1.10 × 10–11
E) 1.11 × 10–9
19. Calculate Kc for the reaction 2HI(g)
H2(g) + I2(g) given that the concentrations of
each species at equilibrium are as follows: [HI] = 0.425 mol/L, [I2] = 0.30 mol/L, [H2] =
0.135 mol/L.
A) 0.22
B) 5.22
C) 22.0
D) 0.19
E) 1.6 × 102
20. Which of the following responses is true with respect to a 0.1 M solution of a weak acid
HA?
A) pH > 1.0
B) pH = 1.0
C) [H+] < [A–]
D) [H+] > [A–]
E) [OH–] > [H+]
21. The acid dissociation constant Ka equals 1.26 × 10–2 for HSO4– is 5.6 × 10–10 for NH4+.
Which statement about the following equilibrium is correct?
HSO4– (aq) + NH3 (aq)
SO42– (aq) + NH4+ (aq)
A) The products will be favored because the hydrogen sulfate ion is a stronger acid
than the ammonium ion.
B) The reactants will be favored because ammonia is a stronger base than the sulfate
anion.
C) Neither reactants nor products will be favored because all of the species are weak
acids or bases.
D) The initial concentrations of the hydrogen sulfate ion and ammonia must be known
before any prediction can be made.
E) This reaction is impossible to predict, since the strong acid and the weak base
appear on the same side of the equation.
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22. What is the [H3O+] in a buffer that consists of 0.15 M HCOOH and 0.10 M HCOONa?
[Ka = 1.7 × 10–4]
A) 2.6 × 10–4 M
B) 1.1 × 10–4 M
C) 4.3 × 10–4 M
D) 6.7 × 10–5 M
E) None of these choices is correct.
23. When a weak acid is titrated with a weak base, the pH at the equivalence point
A) is determined by the sizes of Ka and Kb.
B) is equal to 7.0.
C) is less than 7.0.
D) is greater than 7.0.
E) is no longer affected by addition of base.
24. Which of the following conditions must be seen for a chemical reaction to be
spontaneous at all temperatures?
A) S° > 0, H° < 0
B) S° > 0, H° > 0
C) S° < 0, H° < 0
D) S° < 0, H° > 0
E) It is not possible for a reaction to be spontaneous at all temperatures.
25. Calculate G° for the following reaction
SiCl4(g) + 2Mg(s)  2MgCl2(s) + Si(s)
Substance:
SiCl4(g)
Mg(s)
MgCl2(s)
–616.98
0
–591.79
ΔGf°(kJ/mol):
A) –566.60 kJ
B) 50.38 kJ
C) 25.19 kJ
D) –25.19 kJ
E) 566.60 kJ
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Si(s)
0