Q: Which of the following correctly converts 0.025 kilometers to centimeters using dimensional analysis?

$$0.025 \times \frac{1000\ \text{m}}{1\ \text{km}} \times \frac{100\ \text{cm}}{1\ \text{m}} = 2500\ \text{cm}$$

Q: Which of the following is a correct balanced chemical equation for the combustion of methane ($$\text{CH}_4$$)?

$$\text{CH}_4 + 2\text{O}_2 \rightarrow \text{CO}_2 + 2\text{H}_2\text{O}$$

Q: A student mixes solutions of silver nitrate ($$\text{AgNO}_3) $$and sodium chloride ($$\text{NaCl}). $$What type of reaction occurs and what is the precipitate?

Double displacement; precipitate is $$\text{AgCl}$$

Q: Which of the following is the correct relationship for Dalton's Law of Partial Pressures?

$$P_{\text{total}} = P_1$ + P_2$ + P_3$ + \ldots$$

Question 1

Which of the following correctly converts 0.025 kilometers to centimeters using dimensional analysis?

Accepted Answer

$$0.025 	imes \frac{1000\ 	ext{m}}{1\ 	ext{km}} 	imes \frac{100\ 	ext{cm}}{1\ 	ext{m}} = 2500\ 	ext{cm}$$

Question 2

Which statement best describes the difference between atomic number and mass number?

Accepted Answer

Atomic number is the number of protons; mass number is the sum of protons and neutrons.

Question 3

A compound contains 40.0% carbon, 6.7% hydrogen, and 53.3% oxygen by mass. What is its empirical formula?

Accepted Answer

$$	ext{CH}_2	ext{O}$$

Question 4

Which of the following is a correct balanced chemical equation for the combustion of methane ($$	ext{CH}_4$$)?

Accepted Answer

$$	ext{CH}_4 + 2	ext{O}_2 ightarrow 	ext{CO}_2 + 2	ext{H}_2	ext{O}$$

Question 5

A student mixes solutions of silver nitrate ($$	ext{AgNO}_3) $$and sodium chloride ($$	ext{NaCl}). $$What type of reaction occurs and what is the precipitate?

Accepted Answer

Double displacement; precipitate is $$	ext{AgCl}$$

Question 6

Which of the following ions is most likely to be soluble in water?

Accepted Answer

$$	ext{NaNO}_3$$

Question 7

Which statement best explains why fluorine has a higher electronegativity than chlorine?

Accepted Answer

Fluorine has a smaller atomic radius, so its valence electrons are closer to the nucleus.

Question 8

Which electron configuration represents a neutral atom of sulfur?

Accepted Answer

$$1s^2$$\ $$2s^2$$\ $$2p^6$$\ $$3s^2$$\ $$3p^4$$

Question 9

Which of the following molecules has a bent molecular geometry?

Accepted Answer

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

Question 10

Which intermolecular force is primarily responsible for the high boiling point of water?

Accepted Answer

Hydrogen bonding

Question 11

A sample of gas at 1.00 atm and 273 K occupies 22.4 L. If the temperature is increased to 546 K at constant pressure, what will be the new volume?

Accepted Answer

$$44.8\ 	ext{L}$$

Question 12

Which of the following best describes the kinetic molecular theory of gases?

Accepted Answer

Gas particles are in constant, random motion and collisions are perfectly elastic.

Question 13

Which of the following phase changes is exothermic?

Accepted Answer

Condensation

Question 14

Which statement about ionic compounds is correct?

Accepted Answer

They have high melting points due to strong electrostatic forces.

Question 15

Which of the following is the correct formula for calculating the heat required to raise the temperature of a substance?

Accepted Answer

$$q = mC\Delta T$$

Question 16

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

Accepted Answer

They have completely filled valence electron shells.

Question 17

Which of the following is the correct relationship for Dalton's Law of Partial Pressures?

Accepted Answer

$$P_{	ext{total}} = P_1$ + P_2$ + P_3$ + \ldots$$

Question 18

Which of the following best describes the trend in atomic radius across a period in the periodic table?

Accepted Answer

Atomic radius decreases from left to right.

Question 19

Which of the following is the correct formula for calculating the energy change in a chemical reaction using enthalpy?

Accepted Answer

$$\Delta H = H_{	ext{products}} - H_{	ext{reactants}}$$

General Chemistry I: Final Exam Study Guide (Chapters 1–11)

Guida di studio - Domande di pratica

Study guide - Flashcard