Specific Heat (1 substance) Problems

How much energy, in calories, is required to heat 150 g of water by 2 degrees Celsius?

300 calories

10 g of water receives 400 calories of energy, what is the change in water temperature?

40 degrees Celsius

100 grams of water receives 400 calories of energy, what is the change in the water temperature?

4 degrees Celsius

You just ate a 500 Calorie lunch, that is enough energy to increase the temp. of 500 grams of water by _________ degrees Celsius.

1000

A candy bar has 250 Calories. That amount of energy could increase the temperature of ________g of water by 2,500 degrees Celsius.

100

A piece of candy has 20 Cal/g. If you eat 0.5 grams of the candy, how many Calories will you consume?

10

63,536 J

If 200 grams of water is to be heated from 24.0°C to 100°C to make a cup of tea, how much heat, in joules, must be added? The specific heat of water is 4.18 J/g°C

7.974 g

How many grams of water would require 2200 joules of heat to raise its temperature from 34°C to 100°C? The specific heat of water is 4.18 J/g°C

0.213 J/g°C

A block of aluminum weighing 140 g is cooled from 98.4°C to 62.2°C with the release of 1080 joules of heat. From this data, calculate the specific heat of aluminum.

13,794 J

100.0 mL of 4.0°C water is heated until its temperature is 37°C. If the specific heat of water is 4.18 J/g°C, calculate the amount of heat energy, in joules, needed to cause this rise in temperature.

0.03 J/g°C

A total of 54.0 Joules of heat are observed as 58.3 g of lead is heated from 12.0°C to 42.0°C. From this data, what is the specific heat of lead?

27,912.5 J

The specific heat of wood is 2.03 J/g°C. How much heat, in joules, is needed to convert 550 g of wood at -15.0°C to 10.0°C?

58,050 J

What is the total amount of heat, in joules, needed to change 2.25 kg of silver at 0.0°C to 200.0°C? The specific heat of silver is 0.129 J/g°C

12.10 g

Granite has a specific heat of 800 J/g°C. What mass of granite is needed to store 150,000 J of heat if the temperature of the granite is to be increased by 15.5 °C?

0.0573 J/g°C

What is the specific heat capacity of silver metal if 55.00 g of the metal absorbs 47.3 J of heat and the temperature rises 15.0°C?

4.2 g

What mass of water will change its temperature by 30°C when 525 J of heat is added to it?

37°C

Calculate the initial temperature if 100.0 g of water is cooled until its temperature is 3.5°C and 14000 J were released. The specific heat of water is 4.184 J/g°C.

1.8 J/g°C

Calculate the specific heat of a piece of wood if 1500.0 g of the wood absorbs 67,500 joules of heat, and its temperature changes from 32°C to 57°C.

2.7 J/g°C

When a 100.0 g nugget of pure gold is heated from 35.0°C to 50.0°C, it absorbed 4000.0 J of energy. Calculate the specific heat of gold.

214 J

2.50 g of hydrogen gas is heated from 17.0°C to 23.0°C. The specific heat of hydrogen is 14.267 J/g°C. How much energy, in joules, is absorbed?

2660 J

The temperature of 335 g of water changed from 24.5°C to 26.4°C. How much heat, in joules, did this sample absorb? The specific heat of water is 4.184 J/g°C.

10.4 g

How many grams of water would require 2892 joules of heat to raise its temperature from 34.0°C to 100.0°C? The specific heat of water is 4.184 J/g∙°C.

0.86 g

How many grams of salt did you put in your dinner if the sample raised from 24.3°C to 34.6°C if the salt absorbed 7800 J? The specific heat of salt is 880 J/g°C.

4.5 g

What is the mass of a diamond that is raised by 2.5°C if the specific heat of diamond is .519 J/g°C and it absorbed 5.9 J of energy?

122 J

Gold has a specific heat of 0.129 J/(g×°C). How

many joules of heat energy are required to raise

the temperature of 15 grams of gold from 22 °C to 85°C?

0.06 J/g°C

An unknown substance with a mass of 100 grams

absorbs 1000 J while undergoing a temperature increase of 15 °C. What is the specific heat of the substance?

4515 J

If the temperature of 34.4 g of ethanol increases

from 25 °C to 78.8 °C, how much heat, in joules, has been absorbed by the ethanol? The specific heat of ethanol is 2.44 J/(g×°C)

301 J lost

Graphite has a specific heat of 0.709 J/(g×°C). If a

25 gram piece of graphite is cooled from 35 °C to 18 °C, how much energy, in joules, was lost by the graphite?

130 g

Copper has a specific heat of 0.385 J/(g×°C). A piece

of copper absorbs 5000 J of energy and undergoes a temperature change from 100 °C to 200 °C. What is the mass of the piece of copper?

2.4 J/g°C

45 grams of an unknown substance undergoes a

temperature increase of 38 °C after absorbing

4172.4 Joules. What is the specific heat of the

substance?

3°C

A 40 g sample of water absorbs 500 Joules of energy. How much did the water temperature change? The specific heat of water is 4.18 J/(g×°C).

0.46 J/g°C

A 15.75-g piece of iron absorbs 1086.75 joules of heat energy, and its temperature changes from 25°C to 175°C. Calculate the specific heat capacity of iron.

297 J

How many joules of heat are needed to raise the temperature of 10.0 g of aluminum from 22°C to 55°C, if the specific heat of aluminum is 0.90 J/g°C?

8°C

To what temperature will a 50.0 g piece of glass raise if it absorbs 300 joules of heat and its specific heat capacity is 0.50 J/g°C? The initial temperature of the glass is 20.0°C.

1.8 J/g°C

Calculate the heat capacity of a piece of wood if 1500.0 g of the wood absorbs 6.75×10⁴ joules of heat, and its temperature changes from 32°C to 57°C.

13794 J

100.0 g of 4.0°C water is heated until its temperature is 37°C. If the specific heat of

water is 4.18 J/g°C, calculate the amount of heat energy, in joules, needed to cause this rise in temperature.