Practice Calorimetry (5.3) - Unit 5: Energetics and Thermochemistry - IB 11 Chemistry

Practice: Calorimetry

Lesson 5.3Unit 5: Energetics and Thermochemistry

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9 questions

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6 sample questions

Question 1.
Define calorimetry.
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Think about what it measures.
Question 2.
What does ΔH represent?
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Consider what happens to heat in reactions.
3Question 3.
What is the primary purpose of calorimetry?
- To measure pressure changes
- To measure heat changes
- To measure temperature changes
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Think about what type of energy change it assesses.
4Question 4.
True or False: A bomb calorimeter is used for measurements at constant pressure.
- True
- False
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Consider how the calorimeter is sealed.
Question 5.
Using a coffee-cup calorimeter, 50.0 mL of 1.0 M HCl is mixed with 50.0 mL of 1.0 M NaOH, and the temperature rises from 25.0 °C to 30.0 °C. Calculate ΔH_neut for the reaction, assuming the specific heat of the solution is 4.18 J/(g·°C) and the solution's density is 1.00 g/mL.
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Remember to use the heat capacity and moles of the limiting reactant.
6Question 6.
Using Hess’s Law, determine the enthalpy change for the reaction 2 NO(g) + O₂(g) → 2 NO₂(g) given the following reactions:
1. N₂(g) + O₂(g) → 2 NO(g) with ΔH = +180.5 kJ.
2. 2 NO(g) + O₂(g) → 2 NO₂(g) with ΔH = -112.0 kJ.
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Keep track of the direction of the reactions you combine.

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