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Lesson: Using Calorimetry Measurements

Worksheet • 8 Questions

Q1:

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

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

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

Q2:

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 / β‹… J g C ∘ .

Q3:

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 2 L bottle of water lost more heat because a greater mass of water was cooled.
  • 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 600 mL bottle of water lost more heat because it cooled more quickly.

Q4:

The addition of 3.15 g of B a ( O H ) Β· 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 ∘ C . Assuming the specific heat of the solution and products is 4 . 2 0 / β‹… J g C ∘ , what is the approximate amount of heat absorbed by the reaction?

The reaction can be represented by the following equation:

Q5:

When a 3.00-g sample of K C l was added to 3 . 0 0 Γ— 1 0 2 g of water in a coffee cup calorimeter, the temperature decreased by 1 . 0 5 ∘ 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 / β‹… J g C ∘ .

Q6:

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

Q7:

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 / β‹… J g C ∘ .

Q8:

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

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