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Chapter 7: Problem 69

Classify each of the following as exothermic or endothermic: a. A reaction releases \(550 \mathrm{~kJ}\). b. The energy level of the products is higher than that of the reactants. c. The metabolism of glucose in the body provides energy.

Short Answer

Expert verified
a: exothermic, b: endothermic, c: exothermic

Step by step solution

01

Review Definition of Exothermic and Endothermic Reactions

Exothermic reactions are those that release energy (usually in the form of heat) to the surroundings, while endothermic reactions absorb energy from the surroundings.
02

Analyze Statement (a)

Statement (a) says 'A reaction releases 550 kJ.' Since the reaction releases energy, it is classified as exothermic.
03

Analyze Statement (b)

Statement (b) states 'The energy level of the products is higher than that of the reactants.' This implies that energy is absorbed during the reaction to raise the energy level of the products, so it is classified as endothermic.
04

Analyze Statement (c)

Statement (c) states 'The metabolism of glucose in the body provides energy.' Metabolism of glucose releases energy that the body uses, hence it is classified as exothermic.

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Key Concepts

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

energy release
When we talk about energy release in the context of chemical reactions, we are referring to exothermic reactions. These types of reactions release energy, usually in the form of heat, to their surroundings. For example, when a reaction releases 550 kJ of energy, it is classified as exothermic. This release of energy can be observed in everyday phenomena like burning wood or digesting food. In these cases, energy is given off to the environment, making the surroundings warmer.
energy absorption
Energy absorption is a hallmark of endothermic reactions. These reactions take in energy from their surroundings, usually converting it to stored chemical energy. For instance, in statement (b) from the exercise, when the energy level of the products is higher than that of the reactants, it signifies that energy has been absorbed to form the products. This is why it is an endothermic reaction. Common examples include photosynthesis in plants, where light energy is absorbed to produce glucose, or melting ice, where heat energy is absorbed to convert ice into water.
chemical reactions
Chemical reactions involve the transformation of reactants into products. They are classified into two main types based on energy changes: exothermic and endothermic reactions. In exothermic reactions, such as the metabolism of glucose in the body, energy is released. This released energy powers various bodily functions. Conversely, in endothermic reactions, energy is absorbed from the environment, resulting in products that have higher energy levels than the reactants. Understanding these concepts helps in predicting the behavior of substances in different conditions, which is crucial in fields like chemistry and biochemistry where energy changes play a pivotal role.

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Most popular questions from this chapter

Balance each of the following chemical equations, and identify the type of reaction: (7.4,7.5) a. \(\mathrm{MgCO}_{3}(s) \longrightarrow \mathrm{MgO}(s)+\mathrm{CO}_{2}(g)\) b. \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)\) c. \(\mathrm{Al}(s)+\mathrm{CuCl}_{2}(a q) \longrightarrow \mathrm{AlCl}_{3}(a q)+\mathrm{Cu}(s)\) d. \(\operatorname{AgNO}_{3}(a q)+\mathrm{MgCl}_{2}(a q) \longrightarrow \mathrm{AgCl}_{2}(s)+\mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}(a q)\)

Fatty acids undergo reaction with oxygen gas and form gaseous carbon dioxide and liquid water when utilized for energy in the body. a. Write and balance the equation for the combustion of the fatty acid aqueous capric acid, \(\mathrm{C}_{10} \mathrm{H}_{20} \mathrm{O}_{2}\). b. Write and balance the equation for the combustion of the fatty acid aqueous myristic acid, \(\mathrm{C}_{14} \mathrm{H}_{28} \mathrm{O}_{2}\).

Balance each of the following chemical equations: a. \(\mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{NO}(g)\) b. \(\mathrm{HgO}(s) \stackrel{\Delta}{\longrightarrow} \mathrm{Hg}(l)+\mathrm{O}_{2}(g)\) c. \(\mathrm{Fe}(s)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{Fe}_{2} \mathrm{O}_{3}(s)\) d. \(\mathrm{Na}(s)+\mathrm{Cl}_{2}(g) \longrightarrow \mathrm{NaCl}(s)\)

Gasohol is a fuel containing liquid ethanol \(\left(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}\right)\) that burns in oxygen gas to give carbon dioxide and water gases. (7.4,7.7,7.8) a. Write the balanced chemical equation. b. How many moles of \(\mathrm{O}_{2}\) are needed to completely react with 4.0 moles of \(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O} ?\) c. If a car produces \(88 \mathrm{~g}\) of \(\mathrm{CO}_{2}\), how many grams of \(\mathrm{O}_{2}\) are used up in the reaction? d. If you burn \(125 \mathrm{~g}\) of \(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}\), how many grams of \(\mathrm{CO}_{2}\) and \(\mathrm{H}_{2} \mathrm{O}\) can be produced?

Calculate the molar mass for each of the following: a. \(\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3},\) antiperspirant b. \(\mathrm{KC}_{4} \mathrm{H}_{5} \mathrm{O}_{6},\) cream of tartar c. \(\mathrm{C}_{16} \mathrm{H}_{19} \mathrm{~N}_{3} \mathrm{O}_{5} \mathrm{~S},\) amoxicillin, antibiotic
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