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Chapter 13: Problem 4

As you know, some solution processes are endothermic and others are exothermic. Provide a molecular interpretation for the difference.

Short Answer

Expert verified
Endothermic reactions absorb energy from the environment to break chemical bonds in the reactants, while exothermic reactions release energy because the formed product bonds are stronger than the reactant bonds that were broken, resulting in a release of energy.

Step by step solution

01

Understand Endothermic Reactions

Endothermic reactions are those in which energy (in the form of heat) is absorbed from the environment. On the molecular level, endothermic reactions need heat energy to break the chemical bonds in the reactant molecules, hence enabling a chemical reaction to take place.
02

Understand Exothermic Reactions

Exothermic reactions, on the other hand, are processes that release energy (in the form of heat) into the environment. This happens because the chemical bonds that are formed in forming the products are stronger than the ones broken in the reactants, hence releasing energy. The difference in energy is expelled as heat.
03

Compare the Two

In comparison, the main difference, thus, lies in how energy is used or released in chemical reactions. For endothermic reactions, energy is ingested from the surroundings to facilitate the breaking of bonds, and therefore these reactions usually cool their environment. Exothermic reactions, in contrast, expel energy, causing the surroundings to heat up.

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Most popular questions from this chapter

A mixture of liquids \(A\) and \(B\) exhibits ideal behavior. At \(84^{\circ} \mathrm{C},\) the total vapor pressure of a solution containing 1.2 moles of \(A\) and 2,3 moles of \(B\) is 331 \(\mathrm{mmHg}\). Upon the addition of another mole of \(\mathrm{B}\) to the solution, the vapor pressure increases to 347 \(\mathrm{mmHg}\). Calculate the vapor pressures of pure \(\mathrm{A}\) and \(\mathrm{B}\) at \(84^{\circ} \mathrm{C}\)

Pheromones are compounds secreted by the females of many insect species to attract males. One of these compounds contains \(80.78 \%\) C, \(13.56 \% \mathrm{H}\), and \(5.66 \%\) O. A solution of \(1.00 \mathrm{~g}\) of this pheromone in \(8.50 \mathrm{~g}\) of benzene freezes at \(3.37^{\circ} \mathrm{C}\). What are the molecular formula and molar mass of the compound? (The normal freezing point of pure benzene is \(5.50^{\circ} \mathrm{C}\) ).

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