Worksheet: Using Calorimetry Measurements

In this worksheet, we will practice using the specific heat of a material to calculate the mass, temperature change, or amount of heat exchanged.

Q1:

When 2.0 g of fructose, C 6 H 1 2 O 6 ( ๐‘  ) , a sugar commonly found in fruits, is burned in oxygen in a bomb calorimeter, the temperature of the calorimeter increases by 3 . 1 6 โˆ˜ C . If the heat capacity of the calorimeter and its contents is 9 . 9 0 k J / โˆ˜ C :

Calculate the heat released by this combustion, ๐‘ž , to 2 significant figures?

From the value of ๐‘ž , calculate the molar enthalpy of combustion for fructose to 2 significant figures.

Q2:

The addition of 3.15 g of B a ( O H ) ยท 8 H O 2 2 to a solution of 1.52 g of N H S C N 4 in 100 g of water in a calorimeter caused the temperature to fall by 3 . 1 โˆ˜ C . Assuming the specific heat of the solution and products is 4 . 2 0 / โ‹… J g C โˆ˜ , what is the approximate amount of heat absorbed by the reaction?

The reaction can be represented by the following equation:

Q3:

When a 3.00-g sample of K C l was added to 3 . 0 0 ร— 1 0 ๏Šจ g of water in a coffee cup calorimeter, the temperature decreased by 1 . 0 5 โˆ˜ C . How much heat is involved in the dissolution of the K C l ? Assume that the specific heat of the solution is 4 . 1 8 4 / โ‹… J g C โˆ˜ .

Q4:

To 3 significant figures, how much heat energy is required to heat a 28.4 g ice cube from โˆ’ 2 1 . 0 โˆ˜ C to โˆ’ 2 . 0 โˆ˜ C ? The specific heat capacity of ice is 2 . 1 0 8 / โ‹… J g C โˆ˜

Q5:

How much would the temperature of 285 g of water increase if 36.5 kJ of heat were added? The specific heat capacity of water is 4 . 1 8 4 / โ‹… J g C โˆ˜ .

Q6:

If 14.5 kJ of heat were added to 515 g of liquid water, how much would its temperature increase? Assume that the specific heat of water is 4 . 1 8 6 / โ‹… J g C โˆ˜ .

Q7:

A 600 mL bottle of water at room temperature and a 2 L bottle of water at the same temperature were placed in a refrigerator. After 30 minutes, the 600 mL bottle of water had cooled to the temperature of the refrigerator. An hour later, the 2 L of water had cooled to the same temperature.

Which sample of water lost the most heat?

  • AThe 600 mL bottle of water lost more heat because it cooled more quickly.
  • BThe bottles lost the same amount of heat because they started at the same temperature and finished at the same temperature.
  • CIt is not possible determine which bottle lost the most heat because we do not know the initial temperature and the final temperature of the water.
  • DThe 2 L bottle of water lost more heat because a greater mass of water was cooled.

Q8:

How much energy is required to heat 300 g of water from 4 . 2 โˆ˜ C to 2 5 . 0 โˆ˜ C and immediately evaporate the liquid? Use values of 4.1813 J/gโ‹…K for the specific heat capacity of water and 43.5 kJ/mol for the enthalpy of vaporization.

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