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Chapter 6: Problem 5

These are various forms of energy: chemical, heat, light, mechanical, and electrical. Suggest ways of interconverting these forms of energy.

Short Answer

Expert verified
Chemical energy converts to heat when substances like wood or fuel are burned. Heat energy can be converted to mechanical energy through processes used in steam engines where heat from burning coal is used to produce steam, moving pistons. Mechanical energy transforms to electrical energy in power plants where flowing water or steam's kinetic energy drives a turbine to create electricity. Finally, electrical energy changes to light energy when an electrical bulb is illuminated by flowing electricity through its filament.

Step by step solution

01

Converting Chemical to Heat Energy

Chemical energy can be converted into heat energy. This is seen when wood or fuel is burned. The chemical potential energy locked within the bonds of these materials is released as heat when they undergo combustion.
02

Converting Heat to Mechanical Energy

Heat energy can be converted to mechanical energy. An example of this is seen in a steam engine, where the heat from burning coal (chemical energy) is used to produce steam, which moves pistons (mechanical energy).
03

Converting Mechanical to Electrical Energy

Mechanical energy can be converted to electrical energy. This conversion is often seen in power plants where the kinetic energy of flowing water or steam drives a turbine which in turn is used to generate electricity.
04

Converting Electrical to Light Energy

Electrical energy can be converted to light energy. For instance, when electricity flows through the filament of a bulb, it gets heated up and emits light.

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Most popular questions from this chapter

Consider these changes: (a) \(\mathrm{Hg}(l) \longrightarrow \mathrm{Hg}(g)\) (b) \(3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{O}_{3}(g)\) (c) \(\mathrm{CuSO}_{4} \cdot 5 \mathrm{H}_{2} \mathrm{O}(s) \longrightarrow \mathrm{CuSO}_{4}(s)+5 \mathrm{H}_{2} \mathrm{O}(g)\) (d) \(\mathrm{H}_{2}(g)+\mathrm{F}_{2}(g) \longrightarrow 2 \mathrm{HF}(g)\) At constant pressure, in which of the reactions is work done by the system on the surroundings? By the surroundings on the system? In which of them is no work done?

How are the standard enthalpies of an element and a compound determined?

What is the difference between specific heat and heat capacity? What are the units for these two quantities? Which is the intensive property and which is the extensive property?

From the enthalpy of formation for \(\mathrm{CO}_{2}\) and the following information, calculate the standard enthalpy of formation for carbon monoxide (CO). $$ \begin{aligned} \mathrm{CO}(g)+\frac{1}{2} \mathrm{O}_{2}(g) & \longrightarrow \mathrm{CO}_{2}(g) \\ \Delta H^{\circ} &=-283.0 \mathrm{~kJ} / \mathrm{mol} \end{aligned} $$Why can't we obtain it directly by measuring the enthalpy of the following reaction?$$\mathrm{C}(\text { graphite })+\frac{1}{2} \mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}(g)$$

A 3.53-g sample of ammonium nitrate \(\left(\mathrm{NH}_{4} \mathrm{NO}_{3}\right)\) was added to \(80.0 \mathrm{~mL}\) of water in a constantpressure calorimeter of negligible heat capacity. As a result, the temperature of the water decreased from \(21.6^{\circ} \mathrm{C}\) to \(18.1^{\circ} \mathrm{C}\). Calculate the heat of solution \(\left(\Delta H_{\mathrm{soln}}\right)\) of ammonium nitrate.
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