The specific heat capacity of a substance is defined as the amount of energy needed to increase the temperature of 1.000 g of the substance by 1.000 °C. What is the specific heat of water? Be sure to include units of J/g°C.
The specific heat capacity of a substance is defined as the amount of energy needed to increase the temperature of 1.000 g of the substance by 1.000 °C. What is the specific heat of water? Be sure to include units of J/g°C.
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![Specific Heat Capacity
In an experiment to determine the relationship between the temperature change of water and the amount of
heat absorbed by the water, an electrical heater was used to increase the temperature of 1.000 g of H20 by
1.000 °C. The energy required was 4.184 J.
6. How much heat was required to increase the temperature of 1.000 g of H,0 by 1.000 °C?
7. How much heat would be required to increase the temperature of 100.0 g of H;O by 1.000 °C?
8. How much heat would be required to increase the temperature of 1.000 g of H,O by 50.00 °C?
9. The specific heat capacity of a substance is defined as the amount of energy needed to increase the
temperature of 1.000 g of the substance by 1.000 °C. What is the specific heat of water? Be sure to include
units of J/g°C.
10. What is the equation that relates the amount of heat absorbed or released by any substance to the change
in temperature of that substance? Write this equation using the following notation: q = heat, m = mass, AT
= change in temperature, and Cs = specific heat capacity.
11. In preparing dinner, you need a cup of very hot water, which you prepare on your electric stove. You use 80
kJ of electrical energy to heat 250 g of H2O starting at 20 °C. What is the final temperature of the water?
12. An unknown piece of metal weighing 100.0 g is heated to 90.0 °C. It is dropped into 250.0 g of H20 at 20.0
°C. The final temperature of the system was found to be 29.0 °C. Determine the specific heat of the metal
using the fact that the heat lost by the metal must equal the heat absorbed by the water.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb2e1466d-1f0c-4b2b-8d5d-4c40ddbd2a7e%2F78259708-0258-4f0b-91b5-82d2b739d36b%2Fg0xlqcd_processed.png&w=3840&q=75)
Transcribed Image Text:Specific Heat Capacity
In an experiment to determine the relationship between the temperature change of water and the amount of
heat absorbed by the water, an electrical heater was used to increase the temperature of 1.000 g of H20 by
1.000 °C. The energy required was 4.184 J.
6. How much heat was required to increase the temperature of 1.000 g of H,0 by 1.000 °C?
7. How much heat would be required to increase the temperature of 100.0 g of H;O by 1.000 °C?
8. How much heat would be required to increase the temperature of 1.000 g of H,O by 50.00 °C?
9. The specific heat capacity of a substance is defined as the amount of energy needed to increase the
temperature of 1.000 g of the substance by 1.000 °C. What is the specific heat of water? Be sure to include
units of J/g°C.
10. What is the equation that relates the amount of heat absorbed or released by any substance to the change
in temperature of that substance? Write this equation using the following notation: q = heat, m = mass, AT
= change in temperature, and Cs = specific heat capacity.
11. In preparing dinner, you need a cup of very hot water, which you prepare on your electric stove. You use 80
kJ of electrical energy to heat 250 g of H2O starting at 20 °C. What is the final temperature of the water?
12. An unknown piece of metal weighing 100.0 g is heated to 90.0 °C. It is dropped into 250.0 g of H20 at 20.0
°C. The final temperature of the system was found to be 29.0 °C. Determine the specific heat of the metal
using the fact that the heat lost by the metal must equal the heat absorbed by the water.
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