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General Chemistry Fall 2015 ( MCKIM62461 )
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Homework 2 (Chapters 1,2,3, 4­1 and 4­2)
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Homework 2 (Chapters 1,2,3, 4­1 and 4­2)
Due: 9:59am on Friday, October 2, 2015
You will receive no credit for items you complete after the assignment is due. Grading Policy
Chapter 4 Algorithmic Question 4
Description: (a) According to the following balanced reaction, how many moles of Al2O3 are required to
exactly react with vS1 moles of H2O? Al2O3(s) + 3H2O(l) → 2 Al(OH)3(s)...
Part A
According to the following balanced reaction, how many moles of Al2O3 are required to exactly react with 3.22
moles of H2O?
Al2O3(s) + 3H2O(l) → 2 Al(OH)3(s)
ANSWER:
6.44 moles Al2O3
0.805 moles Al2O3
1.07 moles Al2O3
3.22 moles Al2O3
12.9 moles Al2O3
1.61 moles Al2O3
Chapter 4 Multiple Choice Question 4
Description: (a) How many moles of nitrogen are formed when 58.6 g of KNO3 decomposes according to the
following reaction? The molar mass of KNO3 is 101.11 g/mol. 4 KNO3(s) → 2 K2O(s) + 2 N2(g) + 5 O2(g)...
Part A
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How many moles of nitrogen are formed when 58.6 g of KNO3 decomposes according to the following
reaction? The molar mass of KNO3 is 101.11 g/mol.
4 KNO3(s) → 2 K2O(s) + 2 N2(g) + 5 O2(g)
ANSWER:
0.724 mol N2
1.73 mol N2
0.580 mol N2
0.290 mol N2
18.5 mol N2
Chapter 4 Multiple Choice Question 8
Description: (a) Consider the following balanced reaction. How many grams of water are required to form 75.9
g of HNO3? Assume that there is excess NO2 present. The molar masses are as follows: H2O = 18.02 g/mol,
HNO3 = 63.02 g/mol. 3 NO2(g) + H2O(l) → 2...
Part A
Consider the following balanced reaction. How many grams of water are required to form 75.9 g of HNO3?
Assume that there is excess NO2 present. The molar masses are as follows: H2O = 18.02 g/mol, HNO3 =
63.02 g/mol.
3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)
ANSWER:
38.0 g H2O
10.9 g H2O
21.7 g H2O
26.5 g H2O
43.4 g H2O
Chapter 4 Non­Algorithmic Question 1
Description: (a) According to the following balanced reaction, how many moles of NO are formed from 8.44
moles of NO2 if there is plenty of water present? 3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)...
Part A
According to the following balanced reaction, how many moles of NO are formed from 8.44 moles of NO2 if
there is plenty of water present?
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3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)
ANSWER:
12.66 moles NO
25.32 moles NO
5.63 moles NO
8.44 moles NO
2.82 moles NO
Chapter 4 Non­Algorithmic Question 17
Description: (a) How many grams of calcium chloride are needed to produce 1.50 g of potassium chloride?
CaCl2(aq) + K2CO3(aq) → 2 KCl(aq) + CaCO3(aq)...
Part A
How many grams of calcium chloride are needed to produce 1.50 g of potassium chloride?
CaCl2(aq) + K2CO3(aq) → 2 KCl(aq) + CaCO3(aq)
ANSWER:
1.12 g
4.47 g
0.896 g
2.23 g
Chapter 4 Multiple Choice Question 15
Description: (a) Determine the limiting reactant (LR) and the mass (in g) of nitrogen that can be formed from
50.0 g N2O4 and 45.0 g N2H4. Some possibly useful molar masses are as follows: N2O4 = 92.02 g/mol, N2H4
= 32.05 g/mol. N2O4(l) + 2 N2H4(l) → 3 N2(g) ...
Part A
Determine the limiting reactant (LR) and the mass (in g) of nitrogen that can be formed from 50.0 g N2O4 and
45.0 g N2H4. Some possibly useful molar masses are as follows: N2O4 = 92.02 g/mol, N2H4 = 32.05 g/mol.
N2O4(l) + 2 N2H4(l) → 3 N2(g) + 4 H2O(g)
ANSWER:
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No LR, 45.0 g N2 formed
LR = N2O4, 105 g N2 formed
LR = N2H4, 13.3 g N2 formed
LR = N2O4, 45.7 g N2 formed
LR = N2H4, 59.0 g N2 formed
Chapter 4 Multiple Choice Question 18
Description: (a) Give the percent yield when 28.16 g of CO2 are formed from the reaction of 4.000 moles of
C8H18 with 4.000 moles of O2. 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O...
Part A
Give the percent yield when 28.16 g of CO2 are formed from the reaction of 4.000 moles of C8H18 with 4.000
moles of O2.
2 C8H18 + 25 O2 → 16 CO2 + 18 H2O
ANSWER:
25.00%
50.00%
12.50%
20.00%
Chapter 4 Non­Algorithmic Question 22
Description: (a) Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg(s) +
O2(g) → 2MgO(s) When 4.00 g of magnesium burns, the theoretical yield of magnesium oxide is ________ g.
Part A
Magnesium burns in air with a dazzling brilliance to produce magnesium oxide:
2Mg(s) + O2(g) → 2MgO(s)
When 4.00 g of magnesium burns, the theoretical yield of magnesium oxide is ________ g.
ANSWER:
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6.63
3.32
13.3
4.00
0.165
Chapter 4 Non­Algorithmic Question 36
Description: (a) 5.0 g of iron is reacted with 5.0 g of water according to the chemical equation shown below.
Which one of the following statements is false? 3 Fe(s) + 4 H2O(l) → Fe3O4(s) + 4 H2(g)...
Part A
5.0 g of iron is reacted with 5.0 g of water according to the chemical equation shown below. Which one of the
following statements is false?
3 Fe(s) + 4 H2O(l) → Fe3O4(s) + 4 H2(g)
ANSWER:
Water is the limiting reactant.
Mass is conserved in this reaction.
2.85 g of H2O are left over.
6.91 g of Fe3O4 are produced.
Chapter 4 Algorithmic Question 41
Description: (a) How many milliliters of a 0.266 M vS1NO3 solution are required to make 150.0 mL of 0.075 M
vS1NO3 solution?
Part A
How many milliliters of a 0.266 M NaNO3 solution are required to make 150.0 mL of 0.075 M NaNO3 solution?
ANSWER:
35.1 mL
42.3 mL
18.8 mL
23.6 mL
53.2 mL
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Chapter 4 Non­Algorithmic Question 39
Description: (a) How many milliliters of a 0.184 M CsNO3 solution contain 0.113 moles of CsNO3?
Part A
How many milliliters of a 0.184 M CsNO3 solution contain 0.113 moles of CsNO3?
ANSWER:
885 mL
543 mL
163 mL
326 mL
614 mL
Chapter 4 Non­Algorithmic Question 49
Description: (a) Determine the concentration of a solution prepared by diluting 20.0 mL of a 0.200 M CsCl to
250.0 mL.
Part A
Determine the concentration of a solution prepared by diluting 20.0 mL of a 0.200 M CsCl to 250.0 mL.
ANSWER:
0.0160 M
0.160 M
0.0320 M
2.50 M
0.00800 M
Chapter 3 Multiple Choice Question 44
Description: (a) Determine the empirical formula for a compound that is found to contain 10.15 mg P and
34.85 mg Cl.
Part A
Determine the empirical formula for a compound that is found to contain 10.15 mg P and 34.85 mg Cl.
ANSWER:
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PCl2
P3Cl
PCl
P2Cl3
PCl3
Chapter 3 Multiple Choice Question 13
Description: (a) Give the name for KMnO4.
Part A
Give the name for KMnO4.
ANSWER:
potassium manganese tetraoxide
potassium permanganate
potassium manganate
potassium permagnesium
potassium magnesate
Chapter 3 Multiple Choice Question 30
Description: (a) How many moles of N2O4 are in 76.3 g N2O4? The molar mass of N2O4 is 92.02 g/mol.
Part A
How many moles of N2O4 are in 76.3 g N2O4? The molar mass of N2O4 is 92.02 g/mol.
ANSWER:
1.00 mole
0.829 moles
7.02 x 103 moles
1.21 moles
1.42 x 10­4 moles
Chapter 2 Multiple Choice Question 45
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Description: (a) What mass (in mg) does 2.63 moles of nickel have?
Part A
What mass (in mg) does 2.63 moles of nickel have?
ANSWER:
1.54 x 105 mg
129 mg
44.8 mg
3.56 x 105 mg
2.23 × 104 mg
Chapter 2 Non­Algorithmic Question 72
Description: (a) How many atoms of nitrogen are in 2.50 moles of NO2?
Part A
How many atoms of nitrogen are in 2.50 moles of NO2?
ANSWER:
1.51 x 1024 atoms
7.53 x 1023 atoms
4.52 x 1024 atoms
3.01 x 1024 atoms
5.02 x 1023 atoms
Chapter 1 Multiple Choice Question 19
Description: (a) Filtration is...
Part A
Filtration is
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a process in which the more volatile liquid is boiled off.
separating a solid from a liquid by pouring off the liquid.
heating a mixture of two solids to fuse them together.
dissolving a solid into a liquid.
pouring a mixture through a filter paper to separate the solid from the liquid.
Chapter 1 Non­Algorithmic Question 39
Description: (a) Determine the mass of an object that has a volume of 88.6 mL and a density of 9.77 g/mL.
Part A
Determine the mass of an object that has a volume of 88.6 mL and a density of 9.77 g/mL.
ANSWER:
866 g
78.8 g
9.07 g
98.37 g
0.110 g
Chapter 3 Multiple Choice Question 33
Description: (a) Calculate the mass percent composition of sulfur in Al2(SO4)3.
Part A
Calculate the mass percent composition of sulfur in Al2(SO4)3.
ANSWER:
42.73 %
28.12 %
9.372 %
35.97 %
21.38 %
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