Question 1

Which of the following statements about dimensional analysis is true?

Accepted Answer

A)  It is a general problem-solving approach that uses the dimensions or units of each value to guide us through calculations. 
B)  It is a problem-solving approach that guides us through calculations without using conversion factors. 
C)  It is a method of calculation that uses graphs for deriving exact values. 
D)  It is a method of calculation that does not require the use of a conversion factor. 
E)  It is a problem-solving approach that takes into consideration the standard deviation values. 
A)  It is a general problem-solving approach that uses the dimensions or units of each value to guide us through calculations. 
B)  It is a problem-solving approach that guides us through calculations without using conversion factors. 
C)  It is a method of calculation that uses graphs for deriving exact values. 
D)  It is a method of calculation that does not require the use of a conversion factor. 
E)  It is a problem-solving approach that takes into consideration the standard deviation values. A

Question 2

Calculate the following: 
$\frac { \left( 1 \times 10 ^ { 120 } \right) \times \left( 1 \times 10 ^ { - 240 } \right) ^ { 4 } } { \left( 1 \times 10 ^ { 300 } \right) ^ { 1 / 3 } }$

Accepted Answer

A)  1 × 10-220 
B)  1 × 10540 
C)  1 × 10-740 
D)  1 × 10-940 
E)  1 × 10-420 
A)  1 × 10-220 
B)  1 × 10540 
C)  1 × 10-740 
D)  1 × 10-940 
E)  1 × 10-420 D

Question 3

Two students independently determine the volume of water delivered by a 10.00-mL pipet. Each student takes 8 measurements, then computes the average volume delivered and the standard deviation. The results are tabulated below. 
$$\begin{array} { l l l } 
& \text { Average } & \text { St. Dev. } \
\hline
\text { Student A } & 10.4 \mathrm {~mL} & \pm 0.7 \mathrm {~mL} \
\text { Student B } & 10.00 \mathrm {~mL} & \pm 0.02 \mathrm {~mL}
\end{array}$$
Which statement best describes the results?

Accepted Answer

A)  A: good precision, good accuracy. B: good precision, good accuracy. 
B)  A: good precision, poor accuracy. B: poor precision, good accuracy. 
C)  A: poor precision, good accuracy. B: good precision, poor accuracy. 
D)  A: poor precision, poor accuracy. B: good precision, good accuracy. 
E)  A: poor precision, poor accuracy. B: poor precision, poor accuracy. 
A)  A: good precision, good accuracy. B: good precision, good accuracy. 
B)  A: good precision, poor accuracy. B: poor precision, good accuracy. 
C)  A: poor precision, good accuracy. B: good precision, poor accuracy. 
D)  A: poor precision, poor accuracy. B: good precision, good accuracy. 
E)  A: poor precision, poor accuracy. B: poor precision, poor accuracy. D

Question 4

As part of the calibration of a new laboratory balance, a solid with a mass of 0.200 g is taken as a standard and determined with the following results: Trial Mass
1 0.197 g
2 0.192 g
3 0.212 g
Average mass: 0.200 g

Accepted Answer

A)  The balance is both accurate and precise. 
B)  The balance is accurate but imprecise. 
C)  The balance is precise but inaccurate. 
D)  The balance is both inaccurate and imprecise. 
E)  None of these 
A)  The balance is both accurate and precise. 
B)  The balance is accurate but imprecise. 
C)  The balance is precise but inaccurate. 
D)  The balance is both inaccurate and imprecise. 
E)  None of these

Question 5

Calcium carbonate, or limestone, is relatively insoluble in water. At 25 °C, only 5.8 mg will dissolve in 1.0 liter of water. What volume of water is needed to dissolve 5.0 g of calcium carbonate?

Accepted Answer

A)  4.6 × 10-3 L 
B)  3.0 × 10-2 L 
C)  1.4 × 102 L 
D)  3.4 × 102 L 
E)  8.6 × 102 L 
A)  4.6 × 10-3 L 
B)  3.0 × 10-2 L 
C)  1.4 × 102 L 
D)  3.4 × 102 L 
E)  8.6 × 102 L

Question 6

Which is the largest mass?

Accepted Answer

A)  10 dg 
B)  10 ng 
C)  10 mg 
D)  10 pg 
E)  10 cg 
A)  10 dg 
B)  10 ng 
C)  10 mg 
D)  10 pg 
E)  10 cg

Question 7

What is the correct answer to the following expression? 8.67 × 10-10 + 6.22 × 10-12

Accepted Answer

A)  8.7322 × 10-10 
B)  8.732 × 10-10 
C)  9 × 10-10 
D)  8.7 × 10-10 
E)  8.73 × 10-10 
A)  8.7322 × 10-10 
B)  8.732 × 10-10 
C)  9 × 10-10 
D)  8.7 × 10-10 
E)  8.73 × 10-10

Question 8

Express the volume 622.8 cm3 in liters.

Accepted Answer

A)  6.228 L 
B)  0.06228 L 
C)  0.6228 L 
D)  62.28 L 
E)  622.8 L 
A)  6.228 L 
B)  0.06228 L 
C)  0.6228 L 
D)  62.28 L 
E)  622.8 L

Question 9

You can identify a metal by carefully determining its density. A 29.51 g sample of an unknown metal is 1.50 cm long, 2.50 cm wide, and 1.00 cm thick. What is the possible identity of the element?

Accepted Answer

A)  Nickel; density = 8.90 g/cm3 
B)  Aluminum; density = 2.70 g/cm3 
C)  Silver; density = 10.5 g/cm3 
D)  Iron; density = 7.87 g/cm3 
E)  Chromium; density = 7.20 g/cm3 
A)  Nickel; density = 8.90 g/cm3 
B)  Aluminum; density = 2.70 g/cm3 
C)  Silver; density = 10.5 g/cm3 
D)  Iron; density = 7.87 g/cm3 
E)  Chromium; density = 7.20 g/cm3

Question 10

Light with a wavelength of 1.5 × 10-8 m is in the X-ray region of the electromagnetic spectrum. What is the wavelength of this light in picometers (pm)?

Accepted Answer

A)  1.5 × 10-80 pm 
B)  1.5 × 10-20 pm 
C)  1.5 × 10-1 pm 
D)  1.5 × 104 pm 
E)  1.5 × 107 pm 
A)  1.5 × 10-80 pm 
B)  1.5 × 10-20 pm 
C)  1.5 × 10-1 pm 
D)  1.5 × 104 pm 
E)  1.5 × 107 pm

Question 11

A student uses a balance to determine the mass of an object as 5.719 grams. The correct mass of the object is 5.586 grams. What is the percent error in the student's mass determination?

Accepted Answer

A)  2.38% 
B)  0.133% 
C)  13.3% 
D)  74.3% 
E)  97.7% 
A)  2.38% 
B)  0.133% 
C)  13.3% 
D)  74.3% 
E)  97.7%

Question 12

Which of the following is the largest volume?

Accepted Answer

A)  5.0 × 102 cm3 
B)  5.0 × 10-4 L 
C)  5.0 × 103 mL 
D)  5.0 × 10-1 L 
E)  5.0 × 105 μL 
A)  5.0 × 102 cm3 
B)  5.0 × 10-4 L 
C)  5.0 × 103 mL 
D)  5.0 × 10-1 L 
E)  5.0 × 105 μL

Question 13

The distance from Austin, Texas, to Lincoln, Nebraska, is 822 miles by car. Which of the following series of calculations will yield this distance in units of kilometers? (1 in = 2.54 cm (exact), 1 mi = 5280 ft (exact), 1 ft = 12 in (exact))

Accepted Answer

A)  $822 \mathrm { mi } \times \frac { 5280 \mathrm { ft } } { 1 \mathrm { mi } } \times \frac { 1 \mathrm { ft } } { 12 \mathrm { in } } \times \frac { 2.54 \mathrm {~cm} } { 1 \mathrm { in } } \times \frac { 100 \mathrm {~m} } { 1 \mathrm {~cm} } \times \frac { 1 \mathrm {~km} } { 1000 \mathrm {~m} }$ 
B)  $822 \mathrm { mi } \times \frac { 12 \mathrm { ft } } { 1 \mathrm { in } } \times \frac { 1 \mathrm { in } } { 2.54 \mathrm {~cm} } \times \frac { 1760 \mathrm { yd } } { 1 \mathrm { mi } } \times \frac { 1 \mathrm {~km} } { 1000 \mathrm {~m} }$ 
C)  $822 \mathrm { mi } \times \frac { 5280 \mathrm { ft } } { 1 \mathrm { mi } } \times \frac { 12 \mathrm { ft } } { 1 \mathrm { in } } \times \frac { 1 \mathrm {~cm} } { 2.54 \mathrm { in } } \times \frac { 1 \mathrm {~m} } { 100 \mathrm {~cm} } \times \frac { 1 \mathrm {~km} } { 1000 \mathrm {~m} }$ 
D)  $822 \mathrm { mi } \times \frac { 5280 \mathrm { ft } } { 1 \mathrm { mi } } \times \frac { 12 \mathrm { in } } { 1 \mathrm { ft } } \times \frac { 2.54 \mathrm {~cm} } { 1 \mathrm { in } } \times \frac { 1 \mathrm {~m} } { 100 \mathrm {~cm} } \times \frac { 1 \mathrm {~km} } { 1000 \mathrm {~m} }$ 
E)  $822 \mathrm { mi } \times \frac { 12 \mathrm { in } } { 1 \mathrm { ft } } \times \frac { 2.54 \mathrm {~cm} } { 1 \mathrm { ft } } \times \frac { 1 \mathrm {~km} } { 1000 \mathrm {~m} }$ 
A)  $822 \mathrm { mi } \times \frac { 5280 \mathrm { ft } } { 1 \mathrm { mi } } \times \frac { 1 \mathrm { ft } } { 12 \mathrm { in } } \times \frac { 2.54 \mathrm {~cm} } { 1 \mathrm { in } } \times \frac { 100 \mathrm {~m} } { 1 \mathrm {~cm} } \times \frac { 1 \mathrm {~km} } { 1000 \mathrm {~m} }$ 
B)  $822 \mathrm { mi } \times \frac { 12 \mathrm { ft } } { 1 \mathrm { in } } \times \frac { 1 \mathrm { in } } { 2.54 \mathrm {~cm} } \times \frac { 1760 \mathrm { yd } } { 1 \mathrm { mi } } \times \frac { 1 \mathrm {~km} } { 1000 \mathrm {~m} }$ 
C)  $822 \mathrm { mi } \times \frac { 5280 \mathrm { ft } } { 1 \mathrm { mi } } \times \frac { 12 \mathrm { ft } } { 1 \mathrm { in } } \times \frac { 1 \mathrm {~cm} } { 2.54 \mathrm { in } } \times \frac { 1 \mathrm {~m} } { 100 \mathrm {~cm} } \times \frac { 1 \mathrm {~km} } { 1000 \mathrm {~m} }$ 
D)  $822 \mathrm { mi } \times \frac { 5280 \mathrm { ft } } { 1 \mathrm { mi } } \times \frac { 12 \mathrm { in } } { 1 \mathrm { ft } } \times \frac { 2.54 \mathrm {~cm} } { 1 \mathrm { in } } \times \frac { 1 \mathrm {~m} } { 100 \mathrm {~cm} } \times \frac { 1 \mathrm {~km} } { 1000 \mathrm {~m} }$ 
E)  $822 \mathrm { mi } \times \frac { 12 \mathrm { in } } { 1 \mathrm { ft } } \times \frac { 2.54 \mathrm {~cm} } { 1 \mathrm { ft } } \times \frac { 1 \mathrm {~km} } { 1000 \mathrm {~m} }$

Question 14

A thin sheet of iridium metal that is 2.70 cm by 5.93 cm has a mass of 16.1 g and a thickness of 0.444 mm. What is the density of iridium?

Accepted Answer

A)  22.600 g/cm3 
B)  2.270 g/cm3 
C)  1.14 × 102 g/cm3 
D)  0.044 g/cm3 
E)  0.442 g/cm3 
A)  22.600 g/cm3 
B)  2.270 g/cm3 
C)  1.14 × 102 g/cm3 
D)  0.044 g/cm3 
E)  0.442 g/cm3

Question 15

A graph of number of marbles (y-axis) versus the weight of the marbles (x-axis, grams) is shown to be linear with a trendline of y = 2.7x. What is the weight of the marbles when the number of marbles is 11?

Accepted Answer

A)  29 
B)  0 
C)  3 
D)  10 
E)  4 
A)  29 
B)  0 
C)  3 
D)  10 
E)  4

Question 16

Round 0.00274485 to 1 significant figure.

Accepted Answer

A)  0.00 
B)  0.003 
C)  0.0027 
D)  0.00274 
E)  0.002745 
A)  0.00 
B)  0.003 
C)  0.0027 
D)  0.00274 
E)  0.002745

Question 17

Using the rules of significant figures, calculate the following: $\frac { ( 9.522 + 5.055 ) } { 3.50 } + 0.660$

Accepted Answer

A)  4.825 
B)  4.8249 
C)  4.8 
D)  4.82 
E)  4.82486 
A)  4.825 
B)  4.8249 
C)  4.8 
D)  4.82 
E)  4.82486

Question 18

How many significant figures are there in the number 4.700?

Accepted Answer

A)  1 
B)  5 
C)  3 
D)  4 
E)  2 
A)  1 
B)  5 
C)  3 
D)  4 
E)  2

Question 19

The boiling point of liquid argon is 87.3 K. What is the boiling point in Celsius degrees?

Accepted Answer

A)  189.1 °C 
B)  -185.9 °C 
C)  87.3 °C 
D)  360.5 °C 
E)  -210.7 °C 
A)  189.1 °C 
B)  -185.9 °C 
C)  87.3 °C 
D)  360.5 °C 
E)  -210.7 °C

Question 20

Significant figures allow us to estimate uncertainty in calculated values. In some circumstances, following significant figure rules can lead to estimates of uncertainty that are too high or low. This is the case for the mathematical expression below.
99 × 1.02 = 100.98
Following the rules governing significant figures in multiplication, the answer can be rounded to 1.0 × 102. What is wrong with rounding this answer to two significant figures?

Accepted Answer

Assume that the absolute uncertainty in

Exam 2: Lets Review: the Tools of Quantitative Chemistry

Which of the following statements about dimensional analysis is true?

Calculate the following: (1×10120)×(1×10−240)4(1×10300)1/3\frac { \left( 1 \times 10 ^ { 120 } \right) \times \left( 1 \times 10 ^ { - 240 } \right) ^ { 4 } } { \left( 1 \times 10 ^ { 300 } \right) ^ { 1 / 3 } }(1×10300)1/3(1×10120)×(1×10−240)4​

As part of the calibration of a new laboratory balance, a solid with a mass of 0.200 g is taken as a standard and determined with the following results: Trial Mass 1 0.197 g 2 0.192 g 3 0.212 g Average mass: 0.200 g

Calcium carbonate, or limestone, is relatively insoluble in water. At 25 °C, only 5.8 mg will dissolve in 1.0 liter of water. What volume of water is needed to dissolve 5.0 g of calcium carbonate?

Which is the largest mass?

What is the correct answer to the following expression? 8.67 × 10-10 + 6.22 × 10-12

Express the volume 622.8 cm3 in liters.

You can identify a metal by carefully determining its density. A 29.51 g sample of an unknown metal is 1.50 cm long, 2.50 cm wide, and 1.00 cm thick. What is the possible identity of the element?

Light with a wavelength of 1.5 × 10-8 m is in the X-ray region of the electromagnetic spectrum. What is the wavelength of this light in picometers (pm)?

A student uses a balance to determine the mass of an object as 5.719 grams. The correct mass of the object is 5.586 grams. What is the percent error in the student's mass determination?

Which of the following is the largest volume?

The distance from Austin, Texas, to Lincoln, Nebraska, is 822 miles by car. Which of the following series of calculations will yield this distance in units of kilometers? (1 in = 2.54 cm (exact), 1 mi = 5280 ft (exact), 1 ft = 12 in (exact))

A thin sheet of iridium metal that is 2.70 cm by 5.93 cm has a mass of 16.1 g and a thickness of 0.444 mm. What is the density of iridium?

A graph of number of marbles (y-axis) versus the weight of the marbles (x-axis, grams) is shown to be linear with a trendline of y = 2.7x. What is the weight of the marbles when the number of marbles is 11?

Round 0.00274485 to 1 significant figure.

Using the rules of significant figures, calculate the following: (9.522+5.055)3.50+0.660\frac { ( 9.522 + 5.055 ) } { 3.50 } + 0.6603.50(9.522+5.055)​+0.660

How many significant figures are there in the number 4.700?

The boiling point of liquid argon is 87.3 K. What is the boiling point in Celsius degrees?

Basic Concepts of Chemistry

Atoms, Molecules, and Ions

Chemical Reactions

Stoichiometry: Quantitative Information About Chemical Reactions

Principles of Chemical Reactivity: Energy and Chemical Reactions

The Structure of Atoms

The Structure of Atoms and Periodic Trends

Bonding and Molecular Structure

Bonding and Molecular Structure Orbital Hybridization and Molecular Orbitals

Gases and Their Properties

Intermolecular Forces and Liquids

The Solid State

Solutions and Their Behavior

Chemical Kinetics: the Rates of Chemical Reactions

Principles of Chemical Reactivity: Equilibria

Principles of Chemical Reactivity: the Chemistry of Acids and Bases

Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria

Principles of Chemical Reactivity: Entropy and Free Energy

Principles of Chemical Reactivity: Electron Transfer Reactions

Environmental Chemistry: Earths Environment, Energy, and Sustainability

The Chemistry of the Main Group Elements

The Chemistry of the Transition Elements

Carbon: Not Just Another Element

Biochemistry

Nuclear Chemistry

Filters

Calculate the following: $\frac { \left( 1 \times 10 ^ { 120 } \right) \times \left( 1 \times 10 ^ { - 240 } \right) ^ { 4 } } { \left( 1 \times 10 ^ { 300 } \right) ^ { 1 / 3 } }$

What is the correct answer to the following expression? 8.67 × 10^-10 + 6.22 × 10^-12

Express the volume 622.8 cm³ in liters.

Light with a wavelength of 1.5 × 10^-8 m is in the X-ray region of the electromagnetic spectrum. What is the wavelength of this light in picometers (pm)?

Using the rules of significant figures, calculate the following: $\frac { ( 9.522 + 5.055 ) } { 3.50 } + 0.660$