Q: A 50.0 g sample of water is heated from 25.0°C to 75.0°C. If the specific heat capacity of water is $$4.18 \ \mathrm{J/g\cdot ^\circ C}$$, how much heat is absorbed by the water?

$$q = 50.0 \times 4.18 \times (75.0 - 25.0) = 10,450 \ \mathrm{J}$$

Q: A student measures the mass of a metal block as 45.0 g and its volume as 15.0 mL. What is the density of the block?

$$\text{Density} = \frac{45.0}{15.0} = 3.00 \ \mathrm{g/mL}$$

Q: A gas sample has a pressure of 2.00 atm, a volume of 5.00 L, and a temperature of 300 K. What is the number of moles of gas present? ($$R = 0.0821 \ \mathrm{L\cdot atm/(mol\cdot K)})$$

$$n = \frac{PV}{RT} = \frac{2.00 \times 5.00}{0.0821 \times 300} = 0.406 \ \mathrm{mol}$$

Question 1

A 50.0 g sample of water is heated from 25.0°C to 75.0°C. If the specific heat capacity of water is $$4.18 \ \mathrm{J/g\cdot ^\circ C}$$, how much heat is absorbed by the water?

Accepted Answer

$$q = 50.0 	imes 4.18 	imes (75.0 - 25.0) = 10,450 \ \mathrm{J}$$

Question 2

Which of the following best explains why ice floats on water?

Accepted Answer

Ice is less dense than liquid water due to hydrogen bonding creating an open lattice structure.

Question 3

A mixture of sand and salt can be separated by which sequence of lab techniques?

Accepted Answer

Dissolve in water, filter, evaporate water.

Question 4

Which of the following statements about periodic trends is correct?

Accepted Answer

Atomic radius decreases across a period due to increased nuclear charge.

Question 5

A student measures the mass of a metal block as 45.0 g and its volume as 15.0 mL. What is the density of the block?

Accepted Answer

$$	ext{Density} = \frac{45.0}{15.0} = 3.00 \ \mathrm{g/mL}$$

Question 6

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

Accepted Answer

Hydrogen bonding

Question 7

Which of the following molecules is nonpolar?

Accepted Answer

CO$$_2$$

Question 8

What is the correct Lewis structure for methane (CH$$_4$$)?

Accepted Answer

Central C atom with four single bonds to four H atoms, no lone pairs on C.

Question 9

Which of the following best describes the VSEPR geometry of ammonia (NH$$_3$$)?

Accepted Answer

Trigonal pyramidal

Question 10

A gas sample has a pressure of 2.00 atm, a volume of 5.00 L, and a temperature of 300 K. What is the number of moles of gas present? ($$R = 0.0821 \ \mathrm{L\cdot atm/(mol\cdot K)})$$

Accepted Answer

$$n = \frac{PV}{RT} = \frac{2.00 	imes 5.00}{0.0821 	imes 300} = 0.406 \ \mathrm{mol}$$

Question 11

Which separation technique would be most effective for separating a mixture of ethanol and water?

Accepted Answer

Distillation

Question 12

Which of the following compounds has the highest lattice energy?

Accepted Answer

MgO

Question 13

Which of the following is an example of a physical property?

Accepted Answer

Melting point

Question 14

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

Accepted Answer

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

Question 15

Which of the following is an isomer of C$$_4H$_{10}$$?

Accepted Answer

2-methylpropane

Question 16

A mixture of oxygen and nitrogen gases is in a container. If the total pressure is 1.00 atm and the partial pressure of oxygen is 0.21 atm, what is the partial pressure of nitrogen?

Accepted Answer

$$P_{N_2$} = 1.00 - 0.21 = 0.79 \ \mathrm{atm}$$

Question 17

Which of the following measurements is the most precise?

Accepted Answer

12.345 g

Question 18

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

Accepted Answer

Strong electrostatic forces between oppositely charged ions require a lot of energy to break.

Question 19

Which of the following statements about mixtures is correct?

Accepted Answer

Mixtures can be separated by physical means.

Question 20

Which of the following molecules has a bent molecular geometry?

Accepted Answer

H$$_2O$$

General Chemistry Final Exam Study Guide: Major Topics and Concepts

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