Q: Convert $5.00 \times 10^7\ \mu\mathrm{m}$ to feet. (Given: $1\ \mathrm{in} = 2.54\ \mathrm{cm}$, $1\ \mathrm{ft} = 12\ \mathrm{in}$)

$1.64 \times 10^3\ \mathrm{ft}$

Q: A chemist needs to convert $4.18 \times 10^{15}\ \mathrm{ps}$ (picoseconds) to kiloseconds. What is the correct answer?

$4.18 \times 10^{-6}\ \mathrm{ks}$

Question 1

A student measures the mass of a sample as 12.30 g and its volume as 4.5 mL. What is the density of the sample, reported to the correct number of significant figures?

Accepted Answer

$2.7\ \mathrm{g/mL}$

Question 2

Which of the following statements best describes the difference between accuracy and precision?

Accepted Answer

Accuracy refers to how close measurements are to the true value, while precision refers to how close measurements are to each other.

Question 3

Convert $5.00 	imes 10^7\ \mu\mathrm{m}$ to feet. (Given: $1\ \mathrm{in} = 2.54\ \mathrm{cm}$, $1\ \mathrm{ft} = 12\ \mathrm{in}$)

Accepted Answer

$1.64 	imes 10^3\ \mathrm{ft}$

Question 4

Which of the following numbers contains exactly three significant figures?

Accepted Answer

$0.0300$

Question 5

A patient’s body temperature is measured as $104.0\ ^\circ\mathrm{F}$. What is this temperature in Kelvin? (Use $^\circ\mathrm{C} = (5/9)(^\circ\mathrm{F} - 32)$ and $K = ^\circ\mathrm{C} + 273.15$)

Accepted Answer

$313.7\ \mathrm{K}$

Question 6

Which of the following conversion factors is exact and will NOT limit the number of significant figures in a calculation?

Accepted Answer

$1\ \mathrm{in} = 2.54\ \mathrm{cm}$

Question 7

A sample of lead has a mass of $220.9\ \mathrm{g}$ and a volume of $19.5\ \mathrm{mL}$. What is the density of lead, reported to the correct number of significant figures?

Accepted Answer

$11.33\ \mathrm{g/mL}$

Question 8

Which of the following is the correct result for $37.68 + 108.428 + 6.71862$, rounded to the correct number of significant figures?

Accepted Answer

$152.83$

Question 9

A chemist needs to convert $4.18 	imes 10^{15}\ \mathrm{ps}$ (picoseconds) to kiloseconds. What is the correct answer?

Accepted Answer

$4.18 	imes 10^{-6}\ \mathrm{ks}$

Question 10

Which of the following best describes the rule for significant figures in multiplication and division?

Accepted Answer

The result should have as many significant figures as the number with the fewest significant figures.

Question 11

A nurse needs to administer 250 mL of a solution. How many quarts is this? (Given: $1\ \mathrm{qt} = 0.946\ \mathrm{L}$)

Accepted Answer

$0.264\ \mathrm{qt}$

Question 12

Which of the following is the correct result for $0.80 	imes 63.8$, rounded to the correct number of significant figures?

Accepted Answer

$51$

Question 13

A block of unknown metal has a mass of $74.7\ \mathrm{g}$ and a density of $8.96\ \mathrm{g/cm^3}$. What is its volume, reported to the correct number of significant figures?

Accepted Answer

$8.3\ \mathrm{cm^3}$

Question 14

Which of the following is the correct metric prefix for $10^{-9}$?

Accepted Answer

nano

Question 15

A runner completes a 5.00 mile race. How many kilometers did the runner travel? (Given: $1\ \mathrm{mile} = 5280\ \mathrm{ft}$, $1\ \mathrm{ft} = 12\ \mathrm{in}$, $1\ \mathrm{in} = 2.54\ \mathrm{cm}$, $1\ \mathrm{m} = 100\ \mathrm{cm}$, $1\ \mathrm{km} = 1000\ \mathrm{m}$)

Accepted Answer

$8.05\ \mathrm{km}$

Question 16

Which of the following is an example of an exact number?

Accepted Answer

The number of students in a classroom

Question 17

A laboratory technician needs to prepare $250.0\ \mathrm{mL}$ of a solution. How many liters is this, and how many significant figures should the answer have?

Accepted Answer

$0.250\ \mathrm{L}$, 3 significant figures

Question 18

A student subtracts $8.20$ from $8.7$ and gets $0.50$ on their calculator. What is the correct answer, reported to the correct number of significant figures?

Accepted Answer

$0.5$

Question 19

Which of the following best describes the rule for significant figures in addition and subtraction?

Accepted Answer

The result should have as many decimal places as the number with the fewest decimal places.

Significant Figures, Units, Dimensional Analysis, Temperature, and Density: A General Chemistry Study Guide

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