Q: Which formula is used to calculate the molarity ($$M) of a $$solution?

$$M = \frac{\text{moles of solute}}{\text{volume of solution in liters}}$$

Q: Which equation is used to calculate the percent composition of an element in a compound?

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

Q: Which equation is used to calculate the enthalpy change ($$\Delta H) $$for a reaction using Hess's Law?

$$\Delta H_{\text{reaction}} = \sum \Delta H_{\text{steps}}$$

Question 1

Which of the following best describes the scientific method as applied in chemistry?

Accepted Answer

A process involving observation, hypothesis formation, experimentation, and revision to explain natural phenomena.

Question 2

Which of the following is NOT a primary objective of General Chemistry I as outlined in the syllabus?

Accepted Answer

Memorize all elements and their atomic numbers.

Question 3

A student measures the mass of a sample three times and gets values of 2.50 g, 2.51 g, and 2.49 g. The true mass is 2.80 g. Which statement best describes the measurements?

Accepted Answer

The measurements are precise but not accurate.

Question 4

Which equation correctly relates energy ($$E) to $$frequency ($$
u) $$for electromagnetic radiation?

Accepted Answer

$$E = h 
u$$

Question 5

Which of the following statements about the periodic table is correct?

Accepted Answer

Elements in the same group have similar valence electron configurations.

Question 6

A chemical reaction releases 150 kJ of heat to the surroundings. Which term best describes this process?

Accepted Answer

Exothermic

Question 7

Which formula is used to calculate the molarity ($$M) of a $$solution?

Accepted Answer

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

Question 8

Which of the following best explains why ionic compounds tend to have high melting points?

Accepted Answer

They consist of a lattice of oppositely charged ions held together by strong electrostatic forces.

Question 9

Which equation is used to calculate the percent composition of an element in a compound?

Accepted Answer

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

Question 10

A sample of gas occupies 2.0 L at 1.0 atm and 300 K. What will be its volume at 2.0 atm and 300 K, assuming ideal gas behavior?

Accepted Answer

1.0 L

Question 11

Which of the following is a correct statement about Lewis structures?

Accepted Answer

They represent the arrangement of valence electrons around atoms in a molecule.

Question 12

Which equation is used to calculate the enthalpy change ($$\Delta H) $$for a reaction using Hess's Law?

Accepted Answer

$$\Delta H_{	ext{reaction}} = \sum \Delta H_{	ext{steps}}$$

Question 13

Which quantum number determines the shape of an atomic orbital?

Accepted Answer

Angular momentum quantum number ($$l)$$

Question 14

Which of the following best describes a covalent bond?

Accepted Answer

A bond formed by the sharing of electron pairs between atoms.

Question 15

Which equation is used to relate pressure ($$P$$), volume ($$V$$), temperature ($$T$$), and number of moles ($$n) $$for an ideal gas?

Accepted Answer

$$PV = nRT$$

Question 16

Which of the following is a correct statement about intermolecular forces?

Accepted Answer

London dispersion forces are present in all molecules, regardless of polarity.

Question 17

A student is asked to determine the empirical formula of a compound containing 40.0% carbon, 6.7% hydrogen, and 53.3% oxygen by mass. What is the empirical formula?

Accepted Answer

CH2O

Question 18

Which of the following best explains the difference between a real gas and an ideal gas?

Accepted Answer

Real gases deviate from ideal behavior at high pressures and low temperatures due to intermolecular forces and finite molecular volume.

Question 19

Which equation is used to calculate the energy change ($$q) $$when a substance is heated?

Accepted Answer

$$q = m c \Delta T$$

General Chemistry I (CHEM 1201) - Course Syllabus and Study Guide

Study Guide - Practice Questions

Study Guide - Flashcards