Practice Measurement of Enthalpy Changes (Calorimetry) - 4.1.7 | Chapter 4: Energetics/Thermochemistry | IB Grade 12-Chemistry
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4.1.7 - Measurement of Enthalpy Changes (Calorimetry)

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Learning

Practice Questions

Test your understanding with targeted questions related to the topic.

Question 1

Easy

What is the formula used to calculate heat energy in calorimetry?

💡 Hint: Think of the components involved in measuring energy, mass, and temperature change.

Question 2

Easy

Is the enthalpy change (ΔH) negative for exothermic reactions?

💡 Hint: Remember that these reactions release energy to the surroundings.

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 does ΔH represent in a chemical reaction?

  • Heat released
  • Heat absorbed
  • Both A and B depending on the reaction

💡 Hint: Think of the nature of heat change in chemical reactions.

Question 2

True or False: In calorimetry, a higher temperature indicates an endothermic reaction.

  • True
  • False

💡 Hint: Recall how temperature changes relate to heat exchange.

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Challenge Problems

Push your limits with challenges.

Question 1

A calorimeter absorbs 500 J of heat while dissolving a salt in 150 g of water. Calculate the molar enthalpy change if the molar mass of the salt is 58.5 g/mol. What does the sign of ΔH indicate?

💡 Hint: Consider how to convert grams to moles using molar mass.

Question 2

You conduct an experiment where 100 g of water (specific heat 4.18 J/g°C) cools from 100°C to 25°C after a reaction. Calculate the total heat released, and determine if the reaction is exothermic or endothermic.

💡 Hint: Look for the temperature decrease to help with the sign of ΔH.

Challenge and get performance evaluation