Q: Which of the following is the correct metric equality for the prefix 'kilo'?

$$1\ \text{km} = 1000\ \text{m}$$

Q: A patient receives 250 mL of IV fluid. Convert this volume to liters using dimensional analysis.

$$250\ \text{mL} \times \frac{1\ \text{L}}{1000\ \text{mL}} = 0.25\ \text{L}$$

Q: A metal sample has a mass of 18.0 g and a volume of 6.0 mL. What is its density?

$$\frac{18.0\ \text{g}}{6.0\ \text{mL}} = 3.0\ \text{g/mL}$$

Q: Convert 37°C to Fahrenheit.

$$F = (37 \times \frac{9}{5}) + 32 = 98.6\ ^\circ\text{F}$$

Q: Given the atomic number 17 and mass number 35, how many neutrons are in the atom?

$$35 - 17 = 18\ \text{neutrons}$$

Q: Calculate the molar mass of $$\text{C}_6\text{H}_{12}\text{O}_6 ($$glucose).

$$6 \times 12.01 + 12 \times 1.01 + 6 \times 16.00 = 180.18\ \text{g/mol}$$

Q: Which of the following reactions is an example of oxidation?

$$\text{Fe}^{2+} \rightarrow \text{Fe}^{3+} + e^-$$

Q: A gas occupies 2.0 L at 1.0 atm. If the pressure increases to 4.0 atm at constant temperature, what is the new volume?

$$V_2$$ = \frac{$$P_1$$ $$V_1$$}{$$P_2$$} = \frac{1.0 \times 2.0}{4.0} = 0.5\ \text{L}$$

Q: A solution is prepared by dissolving 10 g of NaCl in 90 g of water. What is the mass percent of NaCl?

$$\frac{10}{10+90} \times 100\% = 10\%$$

Question 1

Which of the following statements best describes the difference between a measured number and an exact number?

Accepted Answer

A measured number is obtained using a measuring instrument and has uncertainty, while an exact number is obtained by counting or defined relationships and has no uncertainty.

Question 2

A student measures the mass of a sample as 0.04560 g. How many significant figures are in this measurement?

Accepted Answer

5

Question 3

Which of the following is the correct metric equality for the prefix 'kilo'?

Accepted Answer

$$1\ 	ext{km} = 1000\ 	ext{m}$$

Question 4

A patient receives 250 mL of IV fluid. Convert this volume to liters using dimensional analysis.

Accepted Answer

$$250\ 	ext{mL} 	imes \frac{1\ 	ext{L}}{1000\ 	ext{mL}} = 0.25\ 	ext{L}$$

Question 5

A metal sample has a mass of 18.0 g and a volume of 6.0 mL. What is its density?

Accepted Answer

$$\frac{18.0\ 	ext{g}}{6.0\ 	ext{mL}} = 3.0\ 	ext{g/mL}$$

Question 6

Which of the following is a heterogeneous mixture?

Accepted Answer

Blood

Question 7

Convert 37°C to Fahrenheit.

Accepted Answer

$$F = (37 	imes \frac{9}{5}) + 32 = 98.6\ ^\circ	ext{F}$$

Question 8

Which element is a metalloid?

Accepted Answer

Silicon (Si)

Question 9

Given the atomic number 17 and mass number 35, how many neutrons are in the atom?

Accepted Answer

$$35 - 17 = 18\ 	ext{neutrons}$$

Question 10

Which type of radiation requires the most shielding to protect against its biological effects?

Accepted Answer

Gamma radiation

Question 11

A radioactive isotope has a half-life of 4 hours. If you start with 80 g, how much remains after 12 hours?

Accepted Answer

10 g

Question 12

Which of the following is the correct formula for magnesium chloride?

Accepted Answer

$$	ext{MgCl}_2$$

Question 13

What is the name of the compound $$	ext{Na}_2	ext{SO}_4$$?

Accepted Answer

Sodium sulfate

Question 14

Which molecule has a bent shape according to VSEPR theory?

Accepted Answer

$$	ext{H}_2	ext{O}$$

Question 15

How many moles of oxygen atoms are in 1 mole of $$	ext{H}_2	ext{SO}_4$$?

Accepted Answer

4

Question 16

Calculate the molar mass of $$	ext{C}_6	ext{H}_{12}	ext{O}_6 ($$glucose).

Accepted Answer

$$6 	imes 12.01 + 12 	imes 1.01 + 6 	imes 16.00 = 180.18\ 	ext{g/mol}$$

Question 17

Which of the following reactions is an example of oxidation?

Accepted Answer

$$	ext{Fe}^{2+} ightarrow 	ext{Fe}^{3+} + e^-$$

Question 18

A chemical reaction releases heat to the surroundings. Which type of reaction is this?

Accepted Answer

Exothermic

Question 19

A gas occupies 2.0 L at 1.0 atm. If the pressure increases to 4.0 atm at constant temperature, what is the new volume?

Accepted Answer

$$V_2$$ = \frac{$$P_1$$ $$V_1$$}{$$P_2$$} = \frac{1.0 	imes 2.0}{4.0} = 0.5\ 	ext{L}$$

Question 20

A solution is prepared by dissolving 10 g of NaCl in 90 g of water. What is the mass percent of NaCl?

Accepted Answer

$$\frac{10}{10+90} 	imes 100\% = 10\%$$

CHEM 10003 Chemical Principles: Chapters 2–9 Study Guide

Study Guide - Practice Questions

Study Guide - Flashcards