Q: Which equation correctly relates the amount of heat ($q$) absorbed or released by a substance to its mass ($m$), specific heat ($c$), and temperature change ($\Delta T$)?

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

Question 1

Which of the following is an example of a homogeneous mixture?

Accepted Answer

Brass (an alloy of copper and zinc)

Question 2

A sample of matter is composed of two or more substances that are physically mixed but not chemically combined. Which classification best describes this sample?

Accepted Answer

Mixture

Question 3

Which of the following changes is a chemical change?

Accepted Answer

Burning a log in a campfire

Question 4

Which statement about the states of matter is correct?

Accepted Answer

Liquids have a definite volume but an indefinite shape.

Question 5

Convert a body temperature of $37.22\ ^\circ\mathrm{C}$ to Kelvin.

Accepted Answer

$310.4\ \mathrm{K}$

Question 6

A 24.8 g sample of metal absorbs 275 J of heat, causing its temperature to rise from $20.2\ ^\circ\mathrm{C}$ to $24.5\ ^\circ\mathrm{C}$. What is the specific heat of the metal in $\mathrm{J}/(\mathrm{g}\cdot^\circ\mathrm{C})$?

Accepted Answer

$2.6\ \mathrm{J}/(\mathrm{g}\cdot^\circ\mathrm{C})$

Question 7

How much heat (in calories) is required to raise the temperature of 16 g of titanium (specific heat $0.125\ \mathrm{cal}/(\mathrm{g}\cdot^\circ\mathrm{C})$) from $36.0\ ^\circ\mathrm{C}$ to $41.3\ ^\circ\mathrm{C}$?

Accepted Answer

$11\ \mathrm{cal}$

Question 8

Which of the following best describes potential energy?

Accepted Answer

Energy stored in a compressed spring

Question 9

A 32.0 g sample of ice at $0\ ^\circ\mathrm{C}$ is melted completely. How much energy (in joules) is required? (Heat of fusion for water = $334\ \mathrm{J}/\mathrm{g}$)

Accepted Answer

$1.07 	imes 10^4\ \mathrm{J}$

Question 10

How many kilojoules of heat are absorbed when 260 g of ice melts at $0\ ^\circ\mathrm{C}$? (Heat of fusion for water = $334\ \mathrm{J}/\mathrm{g}$)

Accepted Answer

$86.8\ \mathrm{kJ}$

Question 11

A 50.0 g sample of steam at $100\ ^\circ\mathrm{C}$ condenses to liquid water at $100\ ^\circ\mathrm{C}$. How much energy (in kJ) is released? (Heat of vaporization for water = $2260\ \mathrm{J}/\mathrm{g}$)

Accepted Answer

$113\ \mathrm{kJ}$

Question 12

Which of the following is a physical property?

Accepted Answer

Boiling point

Question 13

Which of the following best describes a compound?

Accepted Answer

A substance composed of two or more elements always combined in the same proportion

Question 14

A KitKat bar contains 210 nutritional Calories. How many joules of energy does this represent? ($1\ \mathrm{Cal} = 1000\ \mathrm{cal}$, $1\ \mathrm{cal} = 4.184\ \mathrm{J}$)

Accepted Answer

$879,000\ \mathrm{J}$

Question 15

Which of the following is NOT a pure substance?

Accepted Answer

Air

Question 16

Which equation correctly relates the amount of heat ($q$) absorbed or released by a substance to its mass ($m$), specific heat ($c$), and temperature change ($\Delta T$)?

Accepted Answer

$q = m 	imes c 	imes \Delta T$

Question 17

Which of the following best describes a heterogeneous mixture?

Accepted Answer

A mixture in which the composition varies from one part to another and the different parts are visible

Question 18

A person with hypothermia has a body temperature of $34.8\ ^\circ\mathrm{C}$. What is this temperature in degrees Fahrenheit?

Accepted Answer

$94.6\ ^\circ\mathrm{F}$

Question 19

Which of the following is an example of kinetic energy?

Accepted Answer

A car driving on a road

Question 20

Which process requires the greatest amount of energy per gram for water?

Accepted Answer

Vaporizing liquid water at $100\ ^\circ\mathrm{C}$

Chapter 3 – Matter and Energy: Classification, Properties, and Energy Changes

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