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Chapter 6: Problem 9

Describe two exothermic processes and two endothermic processes.

Short Answer

Expert verified
Two exothermic processes are combustion (such as burning wood) and respiration. This is because these processes release heat to the surroundings. Two endothermic processes are photosynthesis and evaporation, since these processes absorb heat from their surroundings.

Step by step solution

01

Identify Examples of Exothermic Processes

First, we'll identify two examples of exothermic processes: 1. Combustion: This is a chemical reaction where a substance reacts with oxygen to produce energy in the form of heat. An example would be burning wood in a fireplace. 2. Respiration: This is the process by which the cells in our body produce energy. It's an exothermic reaction because it releases heat as a by-product, keeping our bodies warm.
02

Identify Examples of Endothermic Processes

Next, we'll identify two examples of endothermic processes: 1. Photosynthesis: This is the process by which plants, some bacteria and protists produce food. They absorb energy in the form of sunlight, and convert carbon dioxide and water into glucose and oxygen. 2. Evaporation: This is the process by which liquid water turns into water vapour. Energy is absorbed from the surroundings to provide the molecules in the liquid with the heat energy they need to escape into the gas state.

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Most popular questions from this chapter

Define these terms: enthalpy, enthalpy of reaction. Under what condition is the heat of a reaction equal to the enthalpy change of the same reaction?

Determine the standard enthalpy of formation of ethanol \(\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right)\) from its standard enthalpy of combustion \((-1367.4 \mathrm{~kJ} / \mathrm{mol})\)

The first step in the industrial recovery of zinc from the zinc sulfide ore is roasting, that is, the conversion of \(\mathrm{ZnS}\) to \(\mathrm{ZnO}\) by heating: $$ \begin{aligned} 2 \mathrm{ZnS}(s)+3 \mathrm{O}_{2}(g) \longrightarrow & 2 \mathrm{ZnO}(s)+2 \mathrm{SO}_{2}(g) \\ & \Delta H_{\mathrm{rxn}}^{\circ}=-879 \mathrm{~kJ} / \mathrm{mol} \end{aligned} $$ Calculate the heat evolved (in kJ) per gram of \(\mathrm{ZnS}\) roasted.

From these data, $$ \begin{aligned} \mathrm{S}(\text { rhombic })+\mathrm{O}_{2}(g) \longrightarrow \mathrm{SO}_{2}(g) \\ \Delta H_{\mathrm{rxn}}^{\circ} &=-296.06 \mathrm{~kJ} / \mathrm{mol} \\ \mathrm{S}(\text { monoclinic })+\mathrm{O}_{2}(g) & \longrightarrow \mathrm{SO}_{2}(g) \\ \Delta H_{\mathrm{rxn}}^{\circ} &=-296.36 \mathrm{~kJ} / \mathrm{mol} \end{aligned} $$ calculate the enthalpy change for the transformation $$ S \text { (rhombic) } \longrightarrow \mathrm{S} \text { (monoclinic) } $$ (Monoclinic and rhombic are different allotropic forms of elemental sulfur.)

Methanol \(\left(\mathrm{CH}_{3} \mathrm{OH}\right)\) is an organic solvent and is also used as a fuel in some automobile engines. From the following data, calculate the standard enthalpy of formation of methanol: $$ \begin{aligned} 2 \mathrm{CH}_{3} \mathrm{OH}(l)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{CO}_{2}(g)+4 \mathrm{H}_{2} \mathrm{O}(l) \\ \Delta H_{\mathrm{rxn}}^{\circ}=-1452.8 \mathrm{~kJ} / \mathrm{mol} \end{aligned} $$
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