Calorimetry
Chemistry ⇒ Thermochemistry and Energetics
Calorimetry starts at 10 and continues till grade 12.
QuestionsToday has an evolving set of questions to continuously challenge students so that their knowledge grows in Calorimetry.
How you perform is determined by your score and the time you take.
When you play a quiz, your answers are evaluated in concept instead of actual words and definitions used.
See sample questions for grade 12
A 10 g sample of a substance absorbs 250 J of heat, causing its temperature to rise by 5°C. Calculate its specific heat capacity.
A 200 g sample of water is cooled from 80°C to 30°C. Calculate the amount of heat lost by the water. (Specific heat capacity of water = 4.18 J/g°C)
A 25 g sample of a metal at 80°C is placed in 50 g of water at 20°C. The final temperature is 22°C. If the specific heat capacity of water is 4.18 J/g°C, calculate the specific heat capacity of the metal.
A 50 g metal block at 100°C is placed in 100 g of water at 25°C. The final temperature is 30°C. If the specific heat capacity of the metal is 0.4 J/g°C, calculate the heat lost by the metal.
A bomb calorimeter is used to determine the heat of combustion of a fuel. The temperature of the calorimeter rises by 2.5°C. If the heat capacity of the calorimeter is 8.0 kJ/°C, calculate the heat released by the combustion.
A calorimeter contains 150 g of water at 20°C. A 50 g piece of metal at 100°C is added. The final temperature is 25°C. If the specific heat capacity of water is 4.18 J/g°C, calculate the heat gained by the water.
A reaction in a calorimeter causes the temperature of the solution to drop. Is the reaction endothermic or exothermic?
A solution releases 500 J of heat to the surroundings. What is the sign of q for the system?
Calculate the heat absorbed when 100 g of water is heated from 25°C to 75°C. (Specific heat capacity of water = 4.18 J/g°C)
Describe how you would determine the specific heat capacity of an unknown metal using a calorimeter.
Describe the main sources of error in a calorimetry experiment.
Describe the steps to calibrate a calorimeter.
Explain the main difference between a coffee cup calorimeter and a bomb calorimeter.
Explain why a bomb calorimeter is suitable for measuring the heat of combustion of fuels.
Explain why it is important to use an insulated container in calorimetry experiments.
In a calorimetry experiment, why is it important to stir the solution?
State the law of conservation of energy as it applies to calorimetry.
The heat change in a reaction is calculated as q = m × c × ΔT. What does each symbol represent?
