Q: A student measures the mass of a sample as 12.34 g and its volume as 4.56 mL. What is the density of the sample, and which equation should be used?

Density is calculated using $$\text{Density} = \frac{\text{Mass}}{\text{Volume}}$$, so the density is $$\frac{12.34}{4.56} = 2.71 g/mL.$$

Q: A reaction requires 2.00 mol of $$\text{H}_2$$ and 1.00 mol of $$\text{O}_2 to $$produce water. If you start with 3.00 mol of $$\text{H}_2$$ and 2.00 mol of $$\text{O}_2$$, what is the limiting reactant and how many moles of water are produced?

Limiting reactant is $$\text{O}_2$$; moles of water produced: 2.00 mol

Q: Which equation correctly represents the calculation of percent composition by mass for an element in a compound?

$$\text{Percent composition} = \frac{\text{mass of element in 1 mol compound}}{\text{molar mass of compound}} \times 100\%$$

Q: Which equation represents the calculation of heat ($$q) $$absorbed or released in a physical or chemical change?

$$q = m \times c \times \Delta T$$

Q: A sample of gas occupies 2.00 L at 1.00 atm and 300 K. If the pressure is increased to 2.00 atm and the temperature is decreased to 150 K, what will be the new volume? (Use the combined gas law.)

$$V_2$$ = \frac{$$V_1$$ \times $$P_1$$ \times $$T_2$$}{$$P_2$$ \times $$T_1$$} = \frac{2.00 \times 1.00 \times 150}{2.00 \times 300} = 0.50$$ L

Question 1

Which of the following best describes the relationship between atomic structure and the periodic table?

Accepted Answer

The periodic table is organized by increasing atomic number, which corresponds to the number of protons and determines the electronic structure of each element.

Question 2

A student measures the mass of a sample as 12.34 g and its volume as 4.56 mL. What is the density of the sample, and which equation should be used?

Accepted Answer

Density is calculated using $$	ext{Density} = \frac{	ext{Mass}}{	ext{Volume}}$$, so the density is $$\frac{12.34}{4.56} = 2.71 g/mL.$$

Question 3

Which of the following is the correct chemical nomenclature for the compound $$	ext{Na}_2	ext{SO}_4$$?

Accepted Answer

Sodium sulfate

Question 4

A reaction requires 2.00 mol of $$	ext{H}_2$$ and 1.00 mol of $$	ext{O}_2 to $$produce water. If you start with 3.00 mol of $$	ext{H}_2$$ and 2.00 mol of $$	ext{O}_2$$, what is the limiting reactant and how many moles of water are produced?

Accepted Answer

Limiting reactant is $$	ext{O}_2$$; moles of water produced: 2.00 mol

Question 5

Which equation correctly represents the calculation of percent composition by mass for an element in a compound?

Accepted Answer

$$	ext{Percent composition} = \frac{	ext{mass of element in 1 mol compound}}{	ext{molar mass of compound}} 	imes 100\%$$

Question 6

Which of the following best describes a strong electrolyte in aqueous solution?

Accepted Answer

A compound that dissociates completely into ions in water, conducting electricity well.

Question 7

Which equation represents the calculation of heat ($$q) $$absorbed or released in a physical or chemical change?

Accepted Answer

$$q = m 	imes c 	imes \Delta T$$

Question 8

Which of the following statements about atomic theory is correct?

Accepted Answer

Atoms of different elements have different numbers of protons, which defines the element.

Question 9

A sample of gas occupies 2.00 L at 1.00 atm and 300 K. If the pressure is increased to 2.00 atm and the temperature is decreased to 150 K, what will be the new volume? (Use the combined gas law.)

Accepted Answer

$$V_2$$ = \frac{$$V_1$$ 	imes $$P_1$$ 	imes $$T_2$$}{$$P_2$$ 	imes $$T_1$$} = \frac{2.00 	imes 1.00 	imes 150}{2.00 	imes 300} = 0.50$$ L

Question 10

Which of the following best explains why water ($$	ext{H}_2	ext{O}) $$has a higher boiling point than methane ($$	ext{CH}_4$$)?

Accepted Answer

Water molecules form hydrogen bonds, which are stronger than the London dispersion forces present in methane.

Question 11

Which of the following is the correct electron configuration for a neutral sodium atom ($$	ext{Na}$$, atomic number 11)?

Accepted Answer

$$1s^2$$\ $$2s^2$$\ $$2p^6$$\ $$3s^1$$

Question 12

Which of the following best describes the difference between ionic and covalent bonding?

Accepted Answer

Ionic bonding involves the transfer of electrons from one atom to another, resulting in charged ions, while covalent bonding involves the sharing of electrons between atoms.

Question 13

A student mixes solutions of $$	ext{AgNO}_3$$ and $$	ext{NaCl}$$, resulting in the formation of a white precipitate. Which equation represents the net ionic equation for this reaction?

Accepted Answer

$$	ext{Ag}^+ (aq) + 	ext{Cl}^- (aq) ightarrow 	ext{AgCl} (s)$$

Question 14

Which of the following statements about the properties of solids, liquids, and gases is correct?

Accepted Answer

Solids have definite shape and volume due to strong intermolecular forces.

Question 15

Which of the following equations is used to calculate the enthalpy change ($$\Delta H) $$for a reaction using bond energies?

Accepted Answer

$$\Delta H = \sum 	ext{Bond energies of bonds broken} - \sum 	ext{Bond energies of bonds formed}$$

Question 16

A patient receives a saline solution containing $$0.90\%$$ $$	ext{NaCl} by $$mass. If the patient receives 500 mL of solution with a density of $$1.00 g/mL$$, how many grams of $$	ext{NaCl}$$ are administered?

Accepted Answer

Total mass = $$500 	ext{ mL} 	imes 1.00 	ext{ g/mL} = 500 	ext{ g}$$; $$	ext{NaCl}$$ mass = $$0.0090 	imes 500 = 4.5 g$$

Question 17

Which of the following best explains why noble gases are chemically inert?

Accepted Answer

Noble gases have completely filled valence electron shells, making them stable and unlikely to react.

Question 18

Which of the following is the correct formula for calculating molarity ($$M) of a $$solution?

Accepted Answer

$$M = \frac{	ext{moles of solute}}{	ext{liters of solution}}$$

General Chemistry I Syllabus and Course Structure – CHEM 124 (Summer 2026)

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