In an exothermic process, the sign of ΔH is what?

Unlock all questions

This demo includes only 20 questions. Upgrade to access hundreds of questions, flashcards, exam simulations, and disable ads.

Full question bankExam simulationsFlashcards
From $9.99Unlock all

Study for the DAT Bootcamp General Chemistry Test. Enhance your skills with detailed questions and explanations. Master exam topics such as atomic structure, chemical reactions, and periodic trends. Prepare confidently for your exam!

Multiple Choice

In an exothermic process, the sign of ΔH is what?

Explanation:
When heat is released by the system, the enthalpy decreases, so ΔH is negative. In an exothermic process, energy exits as heat to the surroundings, meaning the enthalpy of the products is lower than that of the reactants. Since ΔH = H(products) − H(reactants), this results in ΔH < 0. At constant pressure, ΔH essentially equals the heat exchanged with the surroundings, so the observed heat flow is negative as well. An example is combustion, where the reactants start with higher enthalpy and the reaction releases heat, yielding a negative ΔH.

When heat is released by the system, the enthalpy decreases, so ΔH is negative. In an exothermic process, energy exits as heat to the surroundings, meaning the enthalpy of the products is lower than that of the reactants. Since ΔH = H(products) − H(reactants), this results in ΔH < 0. At constant pressure, ΔH essentially equals the heat exchanged with the surroundings, so the observed heat flow is negative as well. An example is combustion, where the reactants start with higher enthalpy and the reaction releases heat, yielding a negative ΔH.

More Multiple Choice Questions
Subscribe

Get the latest from Examzify

You can unsubscribe at any time. Read our privacy policy