Q: Which equation correctly converts 150 J of energy to calories?

$150 \times \frac{1 \text{ cal}}{4.184 \text{ J}}$

Q: Convert 105.8 °F to Celsius using the correct formula.

$T_\text{C} = \frac{T_\text{F} - 32}{1.8}$

Q: Which formula is used to calculate the amount of heat required to change the temperature of a substance?

$\text{Heat} = \text{mass} \times \Delta T \times \text{specific heat}$

Question 1

Which of the following best describes potential energy?

Accepted Answer

Energy stored in chemical bonds or a compressed spring.

Question 2

A person climbs a mountain. Which type of energy is primarily involved in this activity?

Accepted Answer

Kinetic energy, because the person is moving.

Question 3

Which of the following is an example of kinetic energy?

Accepted Answer

A falling object.

Question 4

Which equation correctly converts 150 J of energy to calories?

Accepted Answer

$150 	imes \frac{1 	ext{ cal}}{4.184 	ext{ J}}$

Question 5

A cup of whole milk contains 12 g of carbohydrate, 9 g of fat, and 5 g of protein. What is the total energy content in kilocalories (kcal)?

Accepted Answer

150 kcal

Question 6

Which of the following statements about temperature is TRUE?

Accepted Answer

Temperature is a measure of molecular motion.

Question 7

Convert 105.8 °F to Celsius using the correct formula.

Accepted Answer

$T_	ext{C} = \frac{T_	ext{F} - 32}{1.8}$

Question 8

What is the normal body temperature of 37 °C in kelvins?

Accepted Answer

310 K

Question 9

Which of the following substances has the highest specific heat?

Accepted Answer

Water

Question 10

How much heat (in kJ) is required to raise the temperature of 325 g of water from 15.0 °C to 77.0 °C? (Specific heat of water = $4.184 	ext{ J/g} \cdot 	ext{°C}$)

Accepted Answer

843 kJ

Question 11

Which statement correctly describes the properties of a liquid?

Accepted Answer

Liquids have an indefinite shape but a definite volume.

Question 12

Which process describes the direct change from solid to gas?

Accepted Answer

Sublimation

Question 13

How many calories are needed to melt 15 g of ice at 0 °C? (Heat of fusion for water = $80 	ext{ cal/g}$)

Accepted Answer

1200 cal

Question 14

How many kilocalories (kcal) are released when 50.0 g of steam condenses at 100 °C? (Heat of vaporization for water = $540 	ext{ cal/g}$)

Accepted Answer

27 kcal

Question 15

A flat line on a heating curve represents:

Accepted Answer

A constant temperature.

Question 16

Which of the following best explains why sand in the desert is hot during the day and cool at night?

Accepted Answer

Sand has a low specific heat.

Question 17

To reduce a fever, an infant is packed in 250 g of ice at 0 °C. If the ice melts and warms to body temperature (37.0 °C), how many total calories are removed from the body? (Heat of fusion = $80 	ext{ cal/g}$, specific heat of water = $1.00 	ext{ cal/g} \cdot 	ext{°C}$)

Accepted Answer

29,000 cal

Question 18

Which of the following is TRUE about energy transfer in chemical reactions?

Accepted Answer

There is always some loss of energy, often as heat.

Question 19

Which formula is used to calculate the amount of heat required to change the temperature of a substance?

Accepted Answer

$	ext{Heat} = 	ext{mass} 	imes \Delta T 	imes 	ext{specific heat}$

Energy and Matter: Foundations for GOB Chemistry

Study Guide - Practice Questions

Study Guide - Flashcards