Carrie is trying to figure out the number of calories in a cube of cheese. To do this, she pours 149.5 mL of water into an aluminum can suspended from a ring stand. She takes the temperature of the water, and finds it to be 17.8 degrees Celsius. Then, she places the 5.23 gram cube of cheese under the can and lights it on fire! While the cheese is burning and for a few minutes after it is done, Carrie records the temperature of the water, finding that it levels out at 21.1 degrees Celsius. How many calories of heat were gained by the water? Please answer to the nearest 0.1 calorie.

A piece of unknown metal with a mass of 23.78 g is heated in boiling water to 97.4°C and then dropped into a coffee cup calorimeter containing 72.71 g of water at 13.65°C. When thermal equilibrium is reached, the final temperature is 24.79°C. Calculate the specific heat capacity of the unknown metal. The specific heat of water is 4.184 J/g/°C.   Round your answer to 2 decimal places.

A calorimeter contains 704 mL of water at 24.8°C. A 346 g piece of iron is heated in a Bunsen burner flame, then quickly submerged in the water in the calorimeter. After adding the hot iron, the temperature of the water in the calorimeter rises to a maximum of 41.8°C. Determine the temperature (in °C) to which the piece of iron was heated. Use the following values for your calculations. specific heat of water: 4.184 J/g°C density of water: 1.0 g/mL specific heat of iron: 0.449 J/g°C °C

A chemist carefully measures the amount of heat needed to raise the temperature of a  155.0mg  sample of  C9H10O2  from  46.5°C  to  66.3°C . The experiment shows that  4.80J  of heat are needed. What can the chemist report for the molar heat capacity of  C9H10O2 ? Be sure your answer has the correct number of significant digits. ⋅J⋅mol−1K−1

A hot 122.8 g lump of an unknown substance initially at 154.8 °C is placed in 35.0 mL of water initially at 25.0 °C and the system is allowed to reach thermal equilibrium. The final temperature of the system is 56.9 °C. Using this information and the specific heat values for several metals in the table, identify the unknown substance. Assume no heat is lost to the surroundings. graphite zinc aluminum titanium tungsten rhodium Substance Specific heat (J/(g-°C)) aluminum 0.897 graphite 0.709 rhodium 0.243 titanium 0.523 0.132 0.388 4.184 tungsten zinc water

On a 14.6 oz bag of candy, the manufacturer states that a single 2.00 oz serving is equivalent to 200. kJ. How many Calories are in the bag of candy?

6) Some students plan to measure the amount of Calories in a potato chip. They fill a metal can with 60 milliliters of water at 15 degrees Celslus. They take a 1.9 gram potato chip, place It under the can of water, and set it on fire. After the chip has stopped burning, the temperature of the water has risen to 85 degrees Celslus. The final welght of the burnt chip Is 0.7 grams. How many calorles per gram are in the chip? (Select 1) O 0.5 Cal/gram 1.5 Cal/gram O 2.5 Cal/gram O 3.5 Cal/gram

A chemist carefully measures the amount of heat needed to raise the temperature of a 284.0 mg sample of a pure substance from 51.6 °C to 61.2 °C. The experiment shows that 13. J of heat are needed. What can the chemist report for the specific heat capacity of the substance? Round your answer to 2 significant digits. - 1

How much thermal energy is absorbed by 172.0 grams of water when its temperature increases from 298K to 342K? (the heat capacity of water is 4.184 J/gK.)

Oh no! Billy forgot that his calorimeter should have 2 coffee cups to contain all the heat. If Billy dropped a 25.0 g piece of solid iron (Cs = 0.449 J/g°C) at 398 K in a coffee cup containing 25.0 mL of water at 298K and because of his mistake, 21% of the heat that should be transferred from the iron to the water is lost to the atmosphere, calculate the final temperature of the iron water mixture?