How much heat will be absorbed by a 87.5 g piece of aluminum (specific heat = 0.930 J/g °C) as it changes temperature from 23.0°C to 67.0°C?

The temperature of the cooling water as it leaves the hot engine of an automobile is 240 F. After it passes through the radiator it has a temperature of 175 F. Calculate the amount of heat transferred from the engine to the surroundings by one gallon of water with a specific heat of 4.184 J/g oC.

How much heat is evolved when 1255 g of water condensesto a liquid at 100°C?

How much heat is absorbed by a 44.7-g piece of leadwhen its temperature increases by 65.4°C?

Thermal Interactions Part 1: In an insulated container, you mix 200. g of water at 80C with 100. g of water at 20C. After mixing, the temperature of the water is 60C. a How much did the temperature of the hot water change? How much did the temperature of the cold water change? Compare the magnitudes (positive values) of these changes. b During the mixing, how did the heat transfer occur: from hot water to cold, or from cold water to hot? c What quantity of heat was transferred from one sample to the other? d How does the quantity of heat transferred to or from the hot-water sample compare with the quantity of heat transferred to or from the cold-water sample? e Knowing these relative quantities of heat, why is the temperature change of the cold water greater than the magnitude of the temperature change of the hot water. f A sample of hot water is mixed with a sample of cold water that has twice its mass. Predict the temperature change of each of the samples. g You mix two samples of water, and one increases by 20C, while the other drops by 60C. Which of the samples has less mass? How do the masses of the two water samples compare? h A 7-g sample of hot water is mixed with a 3-g sample of cold water. How do the temperature changes of the two water samples compare? Part 2: A sample of water is heated from 10C to 50C. Can you calculate the amount of heat added to the water sample that caused this temperature change? If not, what information do you need to perform this calculation? Part 3: Two samples of water are heated from 20C to 60C. One of the samples requires twice as much heat to bring about this temperature change as the other. How do the masses of the two water samples compare? Explain your reasoning.

A piece of iron was heated to 95.4C and dropped into a constant-pressure calorimeter containing 284 g of water at 32.2C. The final temperature of the water and iron was 51.9C. Assuming that the calorimeter itself absorbs a negligible amount of heat, what was the mass (in grams) of the piece of iron? The specific heat of iron is 0.449 J/(gC), and the specific heat of water is 4.18 J/(gC).

A 110.-g sample of copper (specific heat capacity = 0.20 J/C g) is heated to 82.4C and then placed in a container of water at 22.3C. The final temperature of the water and copper is 24.9C. What is the mass of the water in the container, assuming that all the heat lost by the copper is gained by the water?

Copper is used in building the integrated circuits, chips, and printed circuit boards for computers. When 228 J of heat are absorbed by 125 g of copper at 22.38C, the temperature rises to 27.12C. What is the specific heat of copper?

The BTU (British thermal unit) is the unit of energy most commonly used in the United States. One joule=9.48104 BTU. What is the specific heat of water in BTU/lbF? (Specific heat of water is 4.18 J/g C.)

How much heat is required to raise the temperature of 100. grams of water from 25C near room temperature to 100.C its boiling point? The specific heat of water is approximately 4.2Jperg-K. a.3.2104J b.32J c.4.2104J d.76J