Q: A 50.0 g sample of a metal absorbs 400 J of heat, causing its temperature to increase from 20.0°C to 36.0°C. What is the specific heat of the metal?

$$\frac{400}{50.0 \times 16.0} = 0.50\ \mathrm{J/g\ ^\circ C}$$

Q: Which equation correctly expresses the relationship for calculating the amount of heat ($$q) $$absorbed or released by a substance?

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

Q: A 255 g sample of copper is heated from 24°C to 185°C. Given the specific heat of copper is $$0.385\ \mathrm{J/g\ ^\circ C}$$, how much energy is required?

$$255 \times 161 \times 0.385 = 15,800\ \mathrm{J}$$

Q: A 24.8 g sample of a metal absorbs 275 J of energy, causing its temperature to rise from 20.2°C to 24.5°C. What is the specific heat of the metal?

$$\frac{275}{24.8 \times 4.3} = 2.6\ \mathrm{J/g\ ^\circ C}$$

Q: A 150 g sample of iron ($$SH = 0.452\ \mathrm{J/g\ ^\circ C}) $$cools from 100°C to 25°C. How much heat is released?

$$150 \times 75 \times 0.452 = 5,085\ \mathrm{J}$$

Question 1

Which of the following best explains why coastal cities tend to have milder temperatures compared to inland cities?

Accepted Answer

Water has a high specific heat, so it absorbs and releases large amounts of heat with little temperature change.

Question 2

A 50.0 g sample of a metal absorbs 400 J of heat, causing its temperature to increase from 20.0°C to 36.0°C. What is the specific heat of the metal?

Accepted Answer

$$\frac{400}{50.0 	imes 16.0} = 0.50\ \mathrm{J/g\ ^\circ C}$$

Question 3

Which of the following substances would heat up the fastest if the same amount of heat is applied to equal masses of each?

Accepted Answer

Gold, $$SH = 0.129\ \mathrm{J/g\ ^\circ C}$$

Question 4

If 100 g of water at 80°C is mixed with 100 g of water at 20°C, what will be the final temperature, assuming no heat is lost to the surroundings?

Accepted Answer

50°C

Question 5

Which equation correctly expresses the relationship for calculating the amount of heat ($$q) $$absorbed or released by a substance?

Accepted Answer

$$q = m 	imes \Delta T 	imes SH$$

Question 6

A 255 g sample of copper is heated from 24°C to 185°C. Given the specific heat of copper is $$0.385\ \mathrm{J/g\ ^\circ C}$$, how much energy is required?

Accepted Answer

$$255 	imes 161 	imes 0.385 = 15,800\ \mathrm{J}$$

Question 7

Why does sand in the desert become very hot during the day and cool rapidly at night?

Accepted Answer

Sand has a low specific heat, so it changes temperature quickly.

Question 8

A 24.8 g sample of a metal absorbs 275 J of energy, causing its temperature to rise from 20.2°C to 24.5°C. What is the specific heat of the metal?

Accepted Answer

$$\frac{275}{24.8 	imes 4.3} = 2.6\ \mathrm{J/g\ ^\circ C}$$

Question 9

Which of the following statements about specific heat is TRUE?

Accepted Answer

Specific heat is the amount of heat needed to raise the temperature of 1 g of a substance by 1°C.

Question 10

If 100 g of aluminum ($$SH = 0.897\ \mathrm{J/g\ ^\circ C}) $$and 100 g of water ($$SH = 4.184\ \mathrm{J/g\ ^\circ C}) $$both absorb 500 J of heat, which will experience the greater temperature change?

Accepted Answer

Aluminum, because it has a lower specific heat.

Question 11

A 150 g sample of iron ($$SH = 0.452\ \mathrm{J/g\ ^\circ C}) $$cools from 100°C to 25°C. How much heat is released?

Accepted Answer

$$150 	imes 75 	imes 0.452 = 5,085\ \mathrm{J}$$

Question 12

Which of the following best describes the units of specific heat in the SI system?

Accepted Answer

$$\mathrm{J/g\ ^\circ C}$$

Question 13

If the specific heat of a substance is high, what does this imply about its temperature change when heat is added?

Accepted Answer

It will experience a small temperature change.

Question 14

A 200 g sample of a substance is heated, and its temperature increases by 10°C. If the specific heat is $$0.500\ \mathrm{J/g\ ^\circ C}$$, how much heat was absorbed?

Accepted Answer

$$200 	imes 10 	imes 0.500 = 1,000\ \mathrm{J}$$

Question 15

Which of the following is a real-world consequence of water's high specific heat?

Accepted Answer

Oceans moderate the climate of nearby land areas.

Question 16

A 75 g sample of silver ($$SH = 0.235\ \mathrm{J/g\ ^\circ C}) is $$heated from 15°C to 65°C. How much energy is required?

Accepted Answer

$$75 	imes 50 	imes 0.235 = 881\ \mathrm{J}$$

Question 17

Which of the following would require the most energy to increase its temperature by 1°C?

Accepted Answer

100 g of water

Question 18

If ocean water cools, what happens to the surrounding air?

Accepted Answer

The air warms as it absorbs heat from the water.

Question 19

A 10.0 g sample of a substance requires 125 J to increase its temperature from 25°C to 50°C. What is the specific heat?

Accepted Answer

$$\frac{125}{10.0 	imes 25} = 0.50\ \mathrm{J/g\ ^\circ C}$$

Matter and Energy: Specific Heat and Its Applications

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