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Chapter 6: Problem 71

What is the relationship between the potential energy of the reactants and products in an exothermic reaction?

Short Answer

Expert verified
In an exothermic reaction, the potential energy of the reactants is higher than that of the products, with the difference representing the energy released to the environment.

Step by step solution

01

Understanding exothermic reactions

An exothermic reaction is a chemical reaction in which heat is released to the surrounding environment. In terms of energy diagrams, this means that the potential energy of the products is lower than that of the reactants.
02

Describing the relationship

In an exothermic reaction, energy, in the form of heat, is liberated. Therefore, the potential energy of the reactants at the beginning of the reaction is higher than that of the products at the end of the reaction. The difference in potential energy between reactants and products is the energy released to the surroundings.

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Key Concepts

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

Potential Energy
Potential energy in chemistry refers to the stored energy in chemical bonds of a substance. It is a form of energy possessed by the particles because of their arrangements and interactions. In an exothermic reaction, this potential energy plays a crucial role.
Exothermic reactions involve a transformation where the potential energy of the reactants changes. At the start, the potential energy is higher due to strong bonds or more unique molecular interactions. During the reaction, these bonds break and re-form into products with lower potential energy. The excess of this potential energy is what is released as heat into the environment.
  • High potential energy indicates strong chemical bonds within the reactants.
  • The released energy from the potential energy difference reflects as heat.
  • Lower potential energy in products signifies more stable bonds post-reaction.
Chemical Reactions
Chemical reactions involve breaking and reformation of bonds in reactant and product molecules. They can be broadly classified into exothermic and endothermic based on heat exchange with surroundings. Exothermic reactions are characterized by the release of energy, leading to a temperature increase in the surroundings.
For instance, when you light a match, the chemical substances in the match head react with oxygen in an exothermic reaction, releasing heat and light.
  • Exothermic reactions are common in nature and various industrial processes, such as combustion and rusting.
  • The energy change in these reactions is due to the decrease in potential energy from reactants to products.
  • These reactions are desirable when heat is needed, such as in warmth generation or cooking.
Energy Diagrams
Energy diagrams are visual representations of the energy changes during a chemical reaction. They help in understanding how energy transitions from reactants to products. On an energy diagram for an exothermic reaction, you'll notice that the potential energy of reactants is shown as higher than the potential energy of the products.
The diagram typically shows a downward slope, indicating the release of energy to the surroundings at each step of the reaction process. The vertical difference between the reactant and product energy levels is the energy released.
  • Exothermic energy diagrams show a peak before declining, representing the activation energy required to initiate the reaction.
  • They are useful in predicting reaction spontaneity and feasibility.
  • Understanding these diagrams enables insight into reaction mechanisms and energy transformations.

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Most popular questions from this chapter

When the reddish-brown mercury(II) oxide, \(\mathrm{Hg} \mathrm{O}\), is heated, it decomposes to its elements, liquid mercury metal and oxygen gas: (a) What is the molar mass of \(\mathrm{Hg} \mathrm{O}\) ? (b) What is the molar mass of \(\mathrm{Hg}\) ? (c) If \(2.00 \mathrm{~g} \mathrm{Hg} \mathrm{O}\) is decomposed to \(\mathrm{Hg}\), predict the mass of the pure Hg metal produced.

A \(2.00-\mathrm{g}\) peanut is burned in a bomb calorimeter containing \(1200 \mathrm{~g}\) of water. The temperature of the water increases from \(25.00^{\circ} \mathrm{C}\) to \(30.25^{\circ} \mathrm{C}\). (a) How much heat, in joules, did the peanut release as it burned? (b) Calculate the heat content in units of calories and Calories. (c) Calculate the energy value in units of \(\mathrm{Cal} / \mathrm{g}\).

In some areas, gasoline is formulated to contain \(15 \%\) ethanol during some seasons. If gasoline releases \(11.4 \mathrm{kcal} / \mathrm{g}\) upon combustion, but ethanol releases only \(7.12 \mathrm{kcal} / \mathrm{g}\), how much less energy in \(\mathrm{kJ} / \mathrm{g}\) is provided by the mixture than by pure gasoline?

A \(5.00-\mathrm{g}\) piece of fat is bumed in a bomb calorimeter containing \(4050 \mathrm{~g}\) of water. The temperature of the water increases by \(12.4^{\circ} \mathrm{C}\). (a) How much heat, in joules, did the fat release as it burned? (b) Calculate the heat content in units of calories and Calories. (c) Calculate the energy value in units of \(\mathrm{Cal} / \mathrm{g}\). (d) Calculate the heat content in units of \(\mathrm{Cal} / \mathrm{mol}\). Assume the fat is all tristearin, a typical fat with the molecular formula \(\mathrm{C}_{57} \mathrm{H}_{10} \mathrm{O}_{6}\).

Ammonia is synthesized commercially from nitrogen gas and hydrogen gas for the production of fertilizers: $$ \mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \longrightarrow 2 \mathrm{NH}_{3}(g) $$ If \(100.0 \mathrm{~g}\) of nitrogen reacts completely with excess hydrogen, and \(34.0 \mathrm{~g}\) of \(\mathrm{NH}_{3}\) are obtained, what is the percent yield of ammonia?
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