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2 cards from this section. Quick, good the night before a test.
What is the purpose of a coffee-cup calorimeter?
Think about what you measure in chemistry related to energy.
State the equation to calculate heat absorbed by the solution.
Identify what each symbol in the equation stands for.
What is the main purpose of using a coffee-cup calorimeter?
Think about what type of energy changes we focus on in reactions.
True or False: The heat absorbed by the solution is equal to the heat released by the reaction.
Consider the sign of heat flow in reactions.
In an experiment, 50 mL of 0.1 M NaOH is mixed with 50 mL of 0.1 M HCl at room temperature. If the temperature rises from 25.0 °C to 30.0 °C, calculate the change in enthalpy assuming complete neutralization of NaOH and HCl. Assume the density of the solution is 1 g/mL and the specific heat capacity is 4.18 J/(g·°C).
Keep track of moles and ensure you convert units correctly.
You perform a calorimetry experiment using 50 g of KNO3 dissolved in 200 g of water. The initial temperature is 25.0 °C, and the final temperature after dissolution is 20.0 °C. Calculate the enthalpy change of dissolution per mole of KNO₃. Molar mass of KNO₃ is 101.1 g/mol.
Remember that when temperature decreases, heat is absorbed by the surroundings.
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