Question 1

A student measures the length of a metal rod as 12.40 cm using a ruler marked to the nearest 0.1 cm. Which statement best describes the uncertainty in this measurement?

Accepted Answer

The uncertainty is in the hundredths place, so the last digit (0) is estimated.

Question 2

Which of the following numbers contains three significant figures?

Accepted Answer

$$0.00450$$

Question 3

A patient receives 250 mg of a medication. How many grams is this? ($$1\,g = 1000\,mg)$$

Accepted Answer

$$0.250\,g$$

Question 4

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

Accepted Answer

The number of students in a classroom

Question 5

A graduated cylinder contains $$35.5\,mL of $$water. After a metal object is added, the water level rises to $$45.0\,mL. If $$the mass of the object is $$80.0\,g$$, what is its density?

Accepted Answer

$$9.41\,g/mL$$

Question 6

Which of the following statements about mass and weight is correct?

Accepted Answer

Mass remains constant regardless of location, but weight changes with gravity.

Question 7

Convert $$5.00$$ kilometers to meters using the correct number of significant figures.

Accepted Answer

$$5000\,m$$

Question 8

A sample of gasoline has a mass of $$700.0\,g$$ and a volume of $$950.0\,mL. $$What is the density of gasoline in $$g/mL$$?

Accepted Answer

$$0.737\,g/mL$$

Question 9

Which metric prefix represents $$1/1,000,000 of a $$unit?

Accepted Answer

micro-

Question 10

A nurse needs to administer $$0.250\,L of $$saline solution. How many milliliters is this? ($$1\,L = 1000\,mL)$$

Accepted Answer

$$250\,mL$$

Question 11

Which of the following best describes the rule for significant figures when multiplying or dividing measured values?

Accepted Answer

The answer should have as many significant figures as the factor with the fewest significant figures.

Question 12

A laboratory technician needs to convert $$3.50\,cm^3$ to milliliters. What is the correct answer?

Accepted Answer

$$3.50\,mL$$

Question 13

A solution has a density of $$1.20\,g/mL. $$What is the mass of $$250.0\,mL of $$this solution?

Accepted Answer

$$300\,g$$

Question 14

Which of the following is NOT a base unit in the SI system?

Accepted Answer

liter

Question 15

A patient’s urine has a specific gravity of $$1.030. If $$the density of water is $$1.00\,g/mL$$, what is the density of the urine?

Accepted Answer

$$1.03\,g/mL$$

Question 16

Which of the following best explains why zeros at the end of a number without a decimal point are not significant?

Accepted Answer

They are placeholders and do not indicate precision.

Question 17

A sample of mercury has a mass of $$27.2\,g$$ and a volume of $$2.00\,mL. $$What is the density of mercury?

Accepted Answer

$$13.6\,g/mL$$

Question 18

A runner completes a $$10.0\,km$$ race. How many meters did the runner travel?

Accepted Answer

$$10,000\,m$$

Question 19

Which of the following is the correct equality for converting between centimeters and meters?

Accepted Answer

$$1\,m = 100\,cm$$

Question 20

A student records a measurement as $$0.00560\,g. $$How many significant figures does this value have?

Accepted Answer

4

Chapter 2: Measurements – Foundations of Quantitative Chemistry

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