Transcript Clicker Questions

Clicker Questions
Chapter 4
Chemical Quantities
and Aqueous
Reactions
Allison Soult
University of Kentucky
© 2014 Pearson Education, Inc.
How many moles of CO2 are produced when 3 moles of
pentane react with excess oxygen?
C5H12(l) + 8O2(g)  5CO2(g) + 6H2O(l)
a)
b)
c)
d)
5 moles
3/5 moles
15 moles
3 moles
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The overall equation involved in photosynthesis is
6 CO2 + 6 H2O  C6H12O6 + 6 O2.
How many grams of glucose (C6H12O6, 180.1 g/mol)
form when 4.40 g of CO2 react?
a)
b)
c)
d)
18.0 g
3.00 g
108 g
0.0167 g
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The rapid decomposition of sodium azide, NaN3, to
its elements is one of the reactions used to inflate
airbags:
2 NaN3 (s)  2 Na (s) + 3 N2 (g)
How many grams of N2 are produced from 6.00 g
of NaN3?
a)
b)
c)
d)
3.88 g
1.72 g
0.138 g
2.59 g
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The overall equation involved in photosynthesis is
6 CO2 + 6 H2O  C6H12O6 + 6 O2.
How many grams of carbon dioxide (CO2) are required
to produce 18.0 g of C6H12O6?
a) 18.0 g
b) 3.00 g
c) 54.0 g
d) 26.4 g
e) 4.40 g
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Ammonia is produced using the Haber process:
3 H2 + N2  2 NH3
Calculate the mass of ammonia produced when 35.0 g
of nitrogen react with 12.5 g of hydrogen.
a)
b)
c)
d)
e)
47.5 g
42.6 g
35.0 g
63.8 g
70.5 g
© 2014 Pearson Education, Inc.
Ammonia is produced using the Haber process:
3 H2 + N2  2 NH3
What percent yield of ammonia is produced from
15.0 kg each of H2 and N2, if 13.7 kg of product are
recovered? Assume the reaction goes to completion.
a)
b)
c)
d)
e)
7.53 × 10–2 %
1.50 × 10–1 %
75.3%
15.0%
16.2%
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What mass of TiCl4 is needed to produce 25.0 g of Ti if
the reaction proceeds with an 82% yield?
TiCl4 + 2Mg  Ti + 2 MgCl2
a)
b)
c)
d)
30.5 g
121 g
99.1 g
81.2 g
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What is the molarity of an aqueous solution containing
22.5 g of sucrose (C12H22O11) in 35.5 mL of solution?
a)
b)
c)
d)
e)
0.0657 M
1.85 × 10–3 M
1.85 M
3.52 M
0.104 M
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Sulfuric acid is found in some types of batteries. What
volume of 3.50 M H2SO4 is required to prepare 250.0 mL
of 1.25 M H2SO4?
a)
b)
c)
d)
e)
17.5 mL
700. mL
89.3 mL
109 mL
None of the above
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A 45.0 mL solution is 0.500 M HCl. What is the
concentration after 25.0 mL of water is added to the
solution? Assume volumes are additive.
a)
b)
c)
d)
0.321 M
0.179 M
0.900 M
0.278 M
© 2014 Pearson Education, Inc.
Which of the following aqueous solutions would
conduct electricity?
a)
b)
c)
d)
e)
AgNO3
C11H22O11 (sucrose)
CH3CH2OH (ethanol)
All of the above
None of the above
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Which of the following compounds will be insoluble
in water?
a)
b)
c)
d)
e)
Ca(OH)2
Na3PO4
CaS
Hg2Cl2
LiF
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What is the maximum number of grams of PbI2
precipitated upon mixing 25.0 mL of 0.150 M KI with
15.0 mL of 0.175 M Pb(NO3)2?
a)
b)
c)
d)
e)
0.864 g
1.73 g
1.21 g
2.07 g
None of the above
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What is the product, if any, when AgNO3 and NaCl react
in aqueous solution?
a)
b)
c)
d)
e)
AgNO3
NaCl
AgCl
NaNO3
No precipitate
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A 25.0 mL sample of H2SO4 is neutralized with NaOH.
What is the concentration of the H2SO4 if 35.0 mL of
0.150 M NaOH are required to completely neutralize
the acid?
a)
b)
c)
d)
e)
0.210 M
0.105 M
0.150 M
0.420 M
None of the above
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What mass, in grams, of sodium bicarbonate, NaHCO3,
is required to neutralize 1000.0 L of 0.350 M H2SO4?
a)
b)
c)
d)
e)
2.94 × 104 g
1.47 × 104 g
5.88 × 104 g
3.50 × 103 g
1.75 × 103 g
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Determine the oxidation number of the red element in
each of the following compounds:
H2PO4–
a)
b)
c)
d)
e)
+6
+5
+5
+5
+6
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+6
+2
+4
+4
+4
+8
+4
+4
+8
+4
SO32–
N2O4
Which of the following is a redox reaction?
a)
b)
c)
d)
e)
HBr (aq) + KOH (aq) → H2O (l) + KBr (aq)
SO3 (g) + H2O (l) → H2SO4 (aq)
HBr (aq) + Na2S (aq) → NaBr (aq) + H2S (g)
NH4+ (aq) + 2 O2 (g) → H2O (l) + NO3– (aq) + 2 H+ (aq)
None of the above
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What is the reducing agent in the following reaction?
Zn + 2 MnO2 + 2 H2O → Zn(OH)2 + 2 MnO(OH)
a)
b)
c)
d)
e)
Zn
MnO2
H2O
Zn(OH)2
MnO(OH)
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