Calorimetry
Chemistry ⇒ Thermochemistry and Energetics
Calorimetry starts at 10 and continues till grade 12.
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See sample questions for grade 11
A 100 g sample of water is heated from 25°C to 35°C. (Specific heat capacity of water = 4.18 J/g°C) Calculate the amount of heat absorbed by the water.
A 200 g sample of a metal at 80°C is placed in 100 g of water at 20°C. The final temperature is 25°C. (Specific heat of water = 4.18 J/g°C) Calculate the heat gained by the water.
A metal block of mass 50 g at 100°C is placed in 100 g of water at 25°C. The final temperature is 30°C. (Specific heat of metal = 0.4 J/g°C, water = 4.18 J/g°C) Calculate the heat lost by the metal.
A reaction in a calorimeter causes the temperature of 150 g of solution to drop by 3°C. (Specific heat = 4.18 J/g°C) Calculate the heat change for the solution.
A student mixes 50 mL of 1 M HCl with 50 mL of 1 M NaOH in a coffee cup calorimeter. The temperature rises from 22°C to 28°C. Assuming the density and specific heat of the solution are the same as water, calculate the heat evolved. (Specific heat of water = 4.18 J/g°C, density = 1 g/mL)
Describe one way to minimize heat loss to the surroundings in a calorimetry experiment.
Describe the difference between a bomb calorimeter and a coffee cup calorimeter.
Describe the steps involved in determining the specific heat capacity of a metal using a calorimeter.
Explain why it is important to stir the solution in a calorimeter during an experiment.
Explain why the mass of the solution is often assumed to be equal to its volume in grams in calorimetry calculations.
State the law of conservation of energy as it applies to calorimetry.
