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Practice Questions
Test your understanding with targeted questions related to the topic.
Question 1
Easy
What is the purpose of a coffee-cup calorimeter?
💡 Hint: Think about what you measure in chemistry related to energy.
Question 2
Easy
State the equation to calculate heat absorbed by the solution.
💡 Hint: Identify what each symbol in the equation stands for.
Practice 4 more questions and get performance evaluation
Interactive Quizzes
Engage in quick quizzes to reinforce what you've learned and check your comprehension.
Question 1
What is the main purpose of using a coffee-cup calorimeter?
- To measure enthalpy change at constant pressure
- To measure pressure changes
- To measure volume changes
💡 Hint: Think about what type of energy changes we focus on in reactions.
Question 2
True or False: The heat absorbed by the solution is equal to the heat released by the reaction.
- True
- False
💡 Hint: Consider the sign of heat flow in reactions.
Solve 1 more question and get performance evaluation
Challenge Problems
Push your limits with challenges.
Question 1
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).
💡 Hint: Keep track of moles and ensure you convert units correctly.
Question 2
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.
💡 Hint: Remember that when temperature decreases, heat is absorbed by the surroundings.
Challenge and get performance evaluation