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Chapter 12: Problem 24

What is the origin of the energy liberated in an exothermic reaction?

Short Answer

Expert verified
Energy in an exothermic reaction originates from the conversion of chemical energy in bonds to thermal energy released as heat.

Step by step solution

01

Identify Exothermic Reaction

An exothermic reaction is a chemical reaction that releases energy by light or heat. Understanding that it releases energy is the first step.
02

Understand Bond Energy

Chemical bonds contain energy. In an exothermic reaction, the energy required to break the bonds in the reactants is less than the energy released when new bonds form in the products.
03

Energy Difference

Calculate the difference in energy between the reactants and the products. This difference is the energy that is released during the reaction.
04

Origin of Energy

The energy liberated in an exothermic reaction comes from the conversion of chemical energy (stored in bonds) into thermal energy (heat).

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

exothermic reaction
An exothermic reaction is a type of chemical reaction that releases energy in the form of light or heat. This is opposite to an endothermic reaction, which absorbs energy. When you touch the container where an exothermic reaction is happening, it feels warm or hot because of the released energy. Simple everyday examples include burning wood, rusting iron, and mixing water with strong acids. To identify an exothermic reaction, simply look for a temperature increase in the surroundings.
chemical bond energy
In chemistry, bonds between atoms store energy. Chemical bond energy refers to this stored energy within the bonds. In an exothermic reaction, the molecules in reactants have bonds that require less energy to break compared to the energy released when new bonds form in the products. When bonds break, they need energy; when new bonds form, they release energy. This energy difference is crucial to understand why an exothermic reaction releases energy. Breaking bonds in reactants consumes less energy, and forming new bonds in products releases more energy, resulting in a net release of energy.
energy conversion
Energy conversion plays a key role in understanding exothermic reactions. In these reactions, chemical energy stored in reactant bonds is converted into thermal energy, which is released as heat. The energy released raises the temperature of the surroundings, making the environment warmer. Here鈥檚 a step-by-step breakdown of the energy conversion process in an exothermic reaction:
  • First, the bonds in the reactants break, requiring minimal energy.
  • Next, new bonds form in the products, releasing a significant amount of energy.
  • The net effect is that more energy is released than consumed, which manifests as heat.
This transformation from chemical energy to thermal energy is the key idea behind the origin of energy in an exothermic reaction.

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Most popular questions from this chapter

What becomes of the electric energy provided in electrolysis? In what device is this energy transformation reversed?

A displacement reaction is an oxidation-reduction reaction in which one element displaces another from solution. In each of the following displacement reactions identify the element that is oxidized and the element that is reduced: $$\begin{array}{l} \mathrm{Zn}+\mathrm{Cu}^{2+} \longrightarrow \mathrm{Zn}^{2+}+\mathrm{Cu} \\ \mathrm{Fe}+2 \mathrm{H}^{+} \longrightarrow \mathrm{Fe}^{2+}+\mathrm{H}_{2} \\\ \mathrm{Cl}_{2}+2 \mathrm{Br}^{-} \longrightarrow 2 \mathrm{Cl}^{-}+\mathrm{Br}_{2} \end{array}$$

How many moles of atomic oxygen are present in \(1 \mathrm{mol}\) of \(\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2} ?\)

The solubility of a gas in a liquid decreases with increasing temperature. From this observation and what you know of how a change in temperature can affect an equilibrium, would you expect that dissolving a gas in a liquid is an exothermic or an endothermic process?

The reaction \(2 \mathrm{SO}_{2}+\mathrm{O}_{2} \longrightarrow 2 \mathrm{SO}_{3}\) is exothermic. (a) How will a rise in temperature affect the yield of \(\mathrm{SO}_{3}\) in an equilibrium mixture of the three gases? (b) Will an increase in pressure raise or lower the yield? (c) In what possible way can the speed of the reaction be increased at moderate temperatures?
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