10165 – CHEM – 131 – Section 001 – Spring 2016 – General Chemistry Lec II
10165 – CHEM – 131 – Section 001 – Spring 2016 – General Chemistry Lec II
Question 1
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All of the following are clues that a chemical reaction has taken place except
The reactant is smaller.
a.A flame occurs.
b.A color change occurs.
c. A solid forms.
Question 2
Question text
Balance the following equation in standard form and determine the sum of the coefficients.
a.6
b.4
c.3
d.14
e.7
Question 3
Question text
Balance this equation using the smallest possible integers, S + HNO3? H2SO4 + NO2 + H2O. What is the coefficient of water.
Select one:
a.2
b.6
c.8
d. 1
e.
Question 4
Question text
When the following equation is balanced using the smallest possible integers, what is the coefficent of oxygen gas?
C7H16(g) + O2(g) ? CO2(g) + H2O(g)
a.5
b.11
c.2
d.14
e.8
Question 5
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True or false? The equation N2 + 3H2? 2NH3 means that 1 g of N2 reacts with 3 g of H2 to form 2 g of NH3.
Question 6
Question text
Which of the following statements is not true of balancing a chemical equation?
Select one:
a.Subscripts in the reactants must be conserved in the products.
b.The law of conservation of matter must be followed.
c.Phases are often shown for each compound but are not critical to balancing an equation.
d.All of the above statements (a-d) are true.
e.Coefficients are used to balance the atoms on both sides.
Question 7
CH4(g) + 2O2(g) ? CO2(g) + 2H2O(g)
Select one:
a.oxidation-reduction
b.two of these
c.synthesis
d. decomposition
e.combustion
Question 8
Question text
Classify the following reaction:
2Mg(s) + O2(g) ? 2MgO(s)
Select one:
a.synthesis
b.oxidation-reduction
c. a-c are all correct.
d.combustion
e.two of the above
Question 9
The equation 2Ag2O(s) ? 4Ag(s) + O2(g) is a(n) ______________ reaction.
Select one:
a.synthesis
b.two of these
c. oxidation-reduction
d.decomposition
e.combustion
Question 10
Question text
The reaction 2K(s) + Br2(l) ? 2KBr(s) is a(n) ______________ reaction.
Select one:
a.acid-base
b.oxidation-reduction
c.precipitation
d. single-replacement
e.double-displacement
Question 11
When the following equation is balanced in standard form, what is the coefficient in front of the H2O?
C8H18(g) + O2(g) CO2(g) + H2O(g)
a.8
b.18
c.16
d.25
e.1
Question 12
Which of the following is a strong acid?
Select one:
a.phosphoric acid
b.acetic acid
c.hydrofluoric acid
d.lactic acid
e.hydrochloric acid
Question 13
Question text
Which of the following statements is not true?
a.Two nonmetals can undergo an oxidation-reduction reaction.
b.A metal-nonmetal reaction involves electron transfer.
c.When two nonmetals react, the compound formed is ionic.
d.A metal-nonmetal reaction can always be assumed to be an oxidation-reduction reaction.
e.When a metal reacts with a nonmetal, an ionic compound is formed.
Question 14
Question text
17.7 g of Mg represents how many moles?
Select one:
a.none of these
b.1.37 mol
c.42.0 mol
d.4.30 × 102 mol
e.0.728 mol
Correct
Question 15
Question text
21.2 g of oxygen contains
a.none of the above
b.1.28 × 1025 oxygen molecules
c.7.98 × 1023 oxygen atoms
d.42 amu
e.1.33 mol of oxygen molecules
Question 16
Question text
45 atoms of calcium weigh
Select one:
a.1.804 × 103 g
b.900 amu
c.900 g
d.1.804 × 103 amu
e.2.71 × 1025 amu
Question 17
Question text
8.55 x 10-3 moles of an unknown compound has a mass of 0.257 g. The compound could be:
Select one:
a.C5H12
b.CH4
c.C3H8
d.C2H6
e.C4H10
Question 18
A 1.73-mole sample of H2O2 weighs
Select one:
a. 31.2 amu
b. 31.2 g
c. 1.73 g
d. 58.8 g
e 35.7 g
Question 19
Question text
A certain compound has an empirical formula of NH2O. Its molar mass is between 55 and 65 g/mol. Its molecular formula is
Select one:
a N2H4O2
b N2H2O2
c NH2O
d not calculable
Question 20
Question text
A certain compound is found to have the percent composition (by mass) of 85.63% C and 14.37% H. The molecular formula contains 3 carbon atoms. How many hydrogen atoms are contained in a molecular of this compound?
Select one:
A 8
b3
c 2
d 4
e 6
Question 21
A compound is composed of element X and hydrogen. Analysis shows the compound to be 80% X by mass, with three times as many hydrogen atoms as X atoms per molecule. Which element is element X?
Select one:
A F
b none of these
c He
d S
e C
22
Calculate the mass of 5.333 moles of silver nitrate.
a.none of these
b.906.1 g
c.820.8 g
d.31.9 g
e.3.139 × 10–2 g
Question 23
Question text
Convert: 3.577 mol K2O = _____________ g K2O
a.26.33
b 3.577
c.337.0
d 3.797 × 10–2
e 2.154 × 1024
Question 24
Convert: 9.41 mol Cu(NO3)2 = ____________ g Cu(NO3)2
Select one:
none of these
b 1.77 × 103
c 1.61 × 103
d 5.02 × 10–2
e 19.9
Question 25
Question text
Determine the percentage composition (by mass) of tin in SnCl2.
Select one:
a.62.6 %
b.77.0 %
c 38.5 %
d 61.5 %
e 18.7 %
Question 26
Question text
The empirical formula of styrene is CH; its molar mass is 104.1 g/mol. What is the molecular formula of styrene?
Select one:
a.C8H8
b.C2H4
c C6H6
d C10H12
Question 27
What is the molar mass of Li3PO4?
Select one:
a 83.79 g/mol
b 115.79 g/mol
c 108.85 g/mol
d 6.02 × 1023 g/mol
e 84.82 g/mol
Question 28
Question text
Which represents the greatest mass?
Select one:
a.1.0 mol P
b.1.0 mol K
c. all the same
d.1.0 mol Al
e.1.0 mol I
Question 29
True or false? One atomic mass unit (amu) is the mass (in grams) of one mole of the substance.
Question 30
True or false? The empirical formula and the molecular formula for a compound cannot be the same.
Question 31
True or false? The mole can be defined as the number equal to the number of oxygen atoms in 32.00 g of oxygen.
Question 32
An excess of Al and 9.7 mol of Br2 are reacted according to the equation
How many moles of AlBr3 will be formed assuming 100% yield?
Select one:
a.4.9 mol
b.6.5 mol
c.9.7 mol
d.14.6 mol
e.3.2 mol
Question 33
Calculate the mass of water produced when 6.25 g of methane, CH4, reacts with an excess of oxygen in the following unbalanced reaction.
Select one:
a. 7.02 g H2O
b 0.78 g H2O
c. 14.0 g H2O
d.2.25 × 102 g H2O
e.0.347 g H2O
Question 34
Consider the equation: . The molar mass of B is 50.0 g/mol. Which of the following statements is true when equal masses of A and B are reacted?
a.If the molar mass of A is less than the molar mass of B, then B must determine how much C is produced.
b. If the molar mass of A is greater than the molar mass of B, then B must determine how much C is produced.
c.If the molar mass of A is greater than the molar mass of B, then A must determine how much C is produced.
d.If the molar mass of A is less than the molar mass of B, then A must determine how much C is produced.
e If the molar mass of A is the same as the molar mass of B, then A and B react in a perfect stoichiometric ratio and both determine how much C is produced.
Question 35
Consider the following unbalanced equation:
How many moles of water are needed to react with 232. g of Al4C3?
a.0.620 mol
b.0.134 mol
c 19.3 mol
d 1.61 mol
e 348. mol
Question 36
Tin(II) fluoride is added to some dental products to help prevent cavities. Manufacturers have to make the tin(II) fluoride first, though, before they can add it to their products.
How many grams of tin(II) fluoride can be made from 58.0 g of hydrogen fluoride if there is plenty of tin available to react?
a. 908. g
B 227. g
c 116. g
d 454. g
e 1.45 g
Question 37
What mass of carbon dioxide will be produced when 12.9 g of butane reacts with an excess of oxygen in the following reaction?
a none of these
b 39.1 g CO2
c 4.88 g CO2
d 78.1 g CO2
e 51.6 g CO2
Question 38
True or false? A balanced chemical equation is one that has the same number of moles of molecules on each side of the equation.
Question 39
Question text
True or false? A mole ratio is used to convert the moles of a starting substance to the moles of a desired substance.
Question 40
Question text
True or false? The equation can be interpreted by saying that 1 mol of N2 reacts with 3 mol of H2 to form 2 mol of NH3.
Question 41
Question text
A hydrogen balloon is at 25oC, 1.00 atm and has a volume of 1.00 L. How many grams of argon gas must be added to the hydrogen balloon to achieve a volume of 3.84 L at constant temperature and pressure?
Select one:
a 4.64 g
b 93.9 g
c none of these
d 6.27 g
e 7.91 g
Question 42
Question text
A sample of an ideal gas containing 0.918 mol is collected at 742 torr pressure and 31°C. Calculate the volume.
Select one:
aL
b 23.5 L
cL
d none of these
e 2.39 L
Question 43
Question text
A sample of oxygen gas (O2) has a volume of 7.86 L at a temperature of 19oC and a pressure of 1.38 atm. Calculate the moles of O2 molecules present in this gas sample.
Select one:
A none of these
B 0.226 mol
C 6.96 mol
D 0.905 mol
E 0.453 mol
Question 44
Question text
An oxygen sample has a volume of 9.77 L at 27°C and 800.0 torr. How many oxygen molecules does it contain?
Question 45
Avogadro’s law states that:
a The volume of a fixed amount of gas is indirectly proportional to its temperature in Kelvin at constant pressure.
b The volume of a fixed amount of gas is inversely proportional to its pressure at constant temperature.
c The total pressure of a mixture of gases is the simple sum of the partial pressure of all of the gaseous compounds.
d Equal amounts of gases occupy the same volume at constant temperature and pressure.
e The volume of a fixed amount of gas is directly proportional to its temperature in Kelvin at constant pressure.
Question 46
Boyle’s law states that:
Select one:
a Equal amounts of gases occupy the same volume at constant temperature and pressure.
b The volume of a fixed amount of gas is inversely proportional to its pressure at constant temperature.
c The volume of a fixed amount of gas is proportional to its pressure at constant temperature.
d The volume of a fixed amount of gas is directly proportional to its temperature in Kelvin at constant pressure.
e The total pressure of a mixture of gases is the simple sum of the partial pressure of all of the gaseous compounds.
Question 47
Question text
Charles’s law states that:
a.The volume of a fixed amount of gas is inversely proportional to its pressure at constant temperature.
b. The total pressure of a mixture of gases is the simple sum of the partial pressure of all of the gaseous compounds.
C The volume of a fixed amount of gas is directly proportional to its temperature in Kelvin at constant pressure.
D The volume of a fixed amount of gas is indirectly proportional to its temperature in Kelvin at constant pressure.
E Equal amounts of gases occupy the same volume at constant temperature and pressure.
Question 48
A solution has [H+] = 4.7 × 10-8M. The pH of this solution is
a.9.80
b.7.33
c.6.01
d. none of these
e.6.67
Question 49
A solution has a pH of 3.66. The pOH of this solution is
Select one:
a.10.34
b.none of these
c.10.24
d.3.76
e. 3.66
Question 50
Question text
A solution where [H+] = 10-13M is ______________.
Select one:
A acidic
B basic
C strongly acidic
d.neutral
e.two of these
Question 51
Question text
Calculate the [H+] in a solution that has a pH of 2.39.
Select one:
aM
b none of these
c 11.61 M
d 2.39 M
eM
Question 52
Question text
What is the pH of a 3.6 M solution of HClO4?
Select one:
a.
0.56
b.
13.44
c.
–0.56
d.
14.56
e.
minus infinity
Question 53
Question text
What is the pH of a solution that has [OH-] = .
Select one:
a.
3.84 M
b.
1.92 M
c.
none of these
d.
10.16 M
e.
6.90 M
Question 54
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Which of the following is not a strong acid?
Select one:
a.
HClO4
b.
H2SO4
c.
CH3COOH
d.
HCl
e.
HNO3
Question 55
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Which of the following statements is/are correct?
Select one:
a.
None of the above statements (a-c) are correct.
b.
In a basic solution, [OH-] > [H+].
c.
All of the above statements (a-c) are correct.
d.
In an acidic solution, [H+] > [OH-].
e.
In a neutral solution, [H+] = [OH-].
Question 56
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Choose the correct Lewis structure for the NH4+ ion.
Select one:
a.
b.
c.
none of these
d.
e.
Question 57
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Consider the drawings below:
Which of the following statements are true?
I. The electrons in each molecule tend to be attracted to the most electronegative element.
II. Each molecular drawing follows the localized electron model.
III. Both HF and CO2 are linear molecules and therefore nonpolar.
IV. The bond angles of NH3 are slightly less than 109.5o because the lone pair compresses the angles between the bonding pairs.
Select one:
a.
II, IV
b.
All of the above statements (I – IV) are correct.
c.
I, III, IV
d.
I, II, III
e.
I, II, IV
Question 58
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How many lone pairs of electrons are in the Lewis structure for compound, HF?
Select one:
a.
3
b.
4
c.
1
d.
0
e.
none of these
Question 59
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How many of the following will have Lewis structures with multiple bonds?
CO, CO2, CO32-, N2, O2
Select one:
a.
2
b.
1
c.
3
d.
5
e.
4
Question 60
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The number of polar covalent bonds in SF4 is
Select one:
a.
none of these
b.
3
c.
2
d.
4
e.
1
Question 61
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Which has a bent structure?
Select one:
a.
NH3
b.
CO2
c.
CaCl2
d.
O2
e.
H2O
Question 62
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Which has a linear structure?
Select one:
a.
SCl2
b.
OF2
c.
CO2
d.
CaCl2
e.
SO2
Question 63
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Which has a planar structure?
Select one:
a.
CO32-
b.
H3O+
c.
CH4
d.
NF3
e.
SO32-
Question 64
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Which has a tetrahedral structure?
Select one:
a.
CO32-
b.
NH3
c.
SO3
d.
CH4
e.
SO32-
Question 65
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Which has a trigonal pyramid structure?
Select one:
a.
NO3-
b.
SO32-
c.
CO32-
d.
CH4
e.
SO3
Question 66
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Which of the following bonds does not have a dipole moment?
Select one:
a.
C-H
b.
B-F
c.
Br-H
d.
F-F
e.
F-H
Question 67
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Which of these has more than one reasonable resonance structure?
Select one:
a.
SiCl4
b.
BH4-
c.
NO3-
d.
N2H4
e.
PH3
Question 68
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True or false? A bond is a force that holds groups of two or more atoms together and makes them function as a unit.
Select one:
True
False
Question 69
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True or false? CH4 has ionic bonds.
Select one:
True
False
Question 70
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True or false? Covalent bonding occurs when a metal reacts with a nonmetal.
Select one:
True
False