In this worksheet, we will practice using the specific heat of a material to calculate the mass, temperature change, or amount of heat exchanged.
When 2.0 g of fructose, , a sugar commonly found in fruits, is burned in oxygen in a bomb calorimeter, the temperature of the calorimeter increases by . If the heat capacity of the calorimeter and its contents is :
Calculate the heat released by this combustion, , to 2 significant figures?
From the value of , calculate the molar enthalpy of combustion for fructose to 2 significant figures.
The addition of 3.15 g of to a solution of 1.52 g of in 100 g of water in a calorimeter caused the temperature to fall by . Assuming the specific heat of the solution and products is , what is the approximate amount of heat absorbed by the reaction?
The reaction can be represented by the following equation:
When a 3.00-g sample of was added to g of water in a coffee cup calorimeter, the temperature decreased by . How much heat is involved in the dissolution of the ? Assume that the specific heat of the solution is .
To 3 significant figures, how much heat energy is required to heat a 28.4 g ice cube from to ? The specific heat capacity of ice is
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 .
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 .
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.
How much energy is required to heat 300 g of water from to and immediately evaporate the liquid? Use values of 4.1813 J/g⋅K for the specific heat capacity of water and 43.5 kJ/mol for the enthalpy of vaporization.