Practice Enthalpy change, ∆rH of a reaction – Reaction Enthalpy - 5.4 | 5. Thermodynamics | CBSE 11 Chemistry Part 1
K12 Students

Academics

AI-Powered learning for Grades 8–12, aligned with major Indian and international curricula.

Professionals

Professional Courses

Industry-relevant training in Business, Technology, and Design to help professionals and graduates upskill for real-world careers.

Games

Interactive Games

Fun, engaging games to boost memory, math fluency, typing speed, and English skills—perfect for learners of all ages.

Typing
Memory
Math
English Adventures
Knowledge

5.4 - Enthalpy change, ∆rH of a reaction – Reaction Enthalpy

Enroll to start learning

You’ve not yet enrolled in this course. Please enroll for free to listen to audio lessons, classroom podcasts and take practice test.

Learning

Practice Questions

Test your understanding with targeted questions related to the topic.

Question 1

Easy

What is the formula for calculating reaction enthalpy?

💡 Hint: Think about the relationship between products and reactants.

Question 2

Easy

Explain what Hess's Law states.

💡 Hint: Consider it like a shortcut to finding enthalpy for complex reactions.

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

Which of the following defines enthalpy change (∆rH)?

  • A measure of heat absorbed during a reaction.
  • The sum of all products formed.
  • The energy required to initiate a reaction.

💡 Hint: Consider which option references heat specifically.

Question 2

True or False: Hess's Law allows us to determine enthalpy changes for reactions that cannot be measured directly.

  • True
  • False

💡 Hint: Does it state you can only measure directly?

Solve 1 more question and get performance evaluation

Challenge Problems

Push your limits with challenges.

Question 1

Calculate the reaction enthalpy for the combustion of butane given: ∆Hf°(C4H10) = -125.6 kJ/mol, ∆Hf°(CO2) = -393.5 kJ/mol, ∆Hf°(H2O) = -285.8 kJ/mol. The reaction is C4H10 + 13/2 O2 → 4CO2 + 5H2O.

💡 Hint: Consider the stoichiometric coefficients in your calculations.

Question 2

Explain how the enthalpy change differs between a reaction done at high versus low temperature, specifically in relation to spontaneity.

💡 Hint: Think about how temperature influences movement.

Challenge and get performance evaluation