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Chapter 6: Problem 1

Define these terms: system, surroundings, open system, closed system, isolated system, thermal energy, chemical energy, potential energy, kinetic energy, law of conservation of energy.

Short Answer

Expert verified
These terms are key concepts in physics. A system is a part of the universe under study, and its surroundings refer to everything else in the universe. An open system can exchange both mass and energy with its surroundings, a closed system can only exchange energy, and an isolated system can't exchange either. Thermal energy is the internal energy of an object due to the kinetic energy of its atoms and molecules, and chemical energy is stored in the bonds between atoms. Potential energy depends on an object's position or state, and kinetic energy depends on its motion. The law of conservation of energy states that energy cannot be created or destroyed, only transformed from one form to another.

Step by step solution

01

Define System

In scientific terms, a system is a part of the universe that is under study. It can be as large as an ecosystem or as small as an atom.
02

Define Surroundings

Surroundings refer to everything else in the universe that is not a part of the system. This includes everything with which the system can potentially interact.
03

Define Open System

An open system is one in which mass and energy can be exchanged with the surroundings.
04

Define Closed System

A closed system is one in which energy can be exchanged with the surroundings, but mass cannot.
05

Define Isolated System

An isolated system is one in which neither mass nor energy can be exchanged with the surroundings. It is essentially closed off from the rest of the universe.
06

Define Thermal Energy

Thermal energy is related to temperature and is the internal energy of an object due to the kinetic energy of its atoms and molecules.
07

Define Chemical Energy

Chemical energy is the energy held in the bonds between atoms in a molecule. It's the energy required to form the bond, and energy is released when the bond is broken.
08

Define Potential Energy

Potential energy is the energy that an object possesses because of its position or state. For instance, an object held at a height has gravitational potential energy.
09

Define Kinetic Energy

Kinetic energy is the energy an object possesses because of its motion. It depends on both the mass and velocity of the object.
10

Define Law of Conservation of Energy

The law of conservation of energy states that energy cannot be created or destroyed - only transformed or transferred from one form to another. This means that the total energy within a closed system remains constant over time.

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Most popular questions from this chapter

Lime is a term that includes calcium oxide \((\mathrm{CaO}\) also called quicklime) and calcium hydroxide \(\left[\mathrm{Ca}(\mathrm{OH})_{2},\right.\) also called slaked lime \(] .\) It is used in the steel industry to remove acidic impurities, in airpollution control to remove acidic oxides such as \(\mathrm{SO}_{2}\), and in water treatment. Quicklime is made industrially by heating limestone \(\left(\mathrm{CaCO}_{3}\right)\) above \(2000^{\circ} \mathrm{C}\) : $$ \begin{aligned} \mathrm{CaCO}_{3}(s) \longrightarrow \mathrm{CaO}(s)+\mathrm{CO}_{2}(g) \\ \Delta H^{\circ} &=177.8 \mathrm{~kJ} / \mathrm{mol} \end{aligned} $$ Slaked lime is produced by treating quicklime with water: $$ \begin{aligned} \mathrm{CaO}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{Ca}(\mathrm{OH})_{2}(s) \\ \Delta H^{\circ} &=-65.2 \mathrm{~kJ} / \mathrm{mol} \end{aligned} $$ The exothermic reaction of quicklime with water and the rather small specific heats of both quicklime \(\left(0.946 \mathrm{~J} / \mathrm{g} \cdot{ }^{\circ} \mathrm{C}\right)\) and slaked lime \(\left(1.20 \mathrm{~J} / \mathrm{g} \cdot{ }^{\circ} \mathrm{C}\right)\) make it hazardous to store and transport lime in vessels made of wood. Wooden sailing ships carrying lime would occasionally catch fire when water leaked into the hold. (a) If a 500 -g sample of water reacts with an equimolar amount of \(\mathrm{CaO}\) (both at an initial temperature of \(\left.25^{\circ} \mathrm{C}\right)\), what is the final temperature of the product, \(\mathrm{Ca}(\mathrm{OH})_{2} ?\) Assume that the product absorbs all of the heat released in the reaction. (b) Given that the standard enthalpies of formation of \(\mathrm{CaO}\) and \(\mathrm{H}_{2} \mathrm{O}\) are \(-635.6 \mathrm{~kJ} / \mathrm{mol}\) and \(-285.8 \mathrm{~kJ} / \mathrm{mol}\), respectively, cal- culate the standard enthalpy of formation of \(\mathrm{Ca}(\mathrm{OH})_{2}\).

Determine the amount of heat (in \(\mathrm{kJ}\) ) given off when \(1.26 \times 10^{4} \mathrm{~g}\) of ammonia are produced according to the equation $$ \begin{aligned} \mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \longrightarrow & 2 \mathrm{NH}_{3}(g) \\\ \Delta H_{\mathrm{rxn}}^{\circ} &=-92.6 \mathrm{~kJ} / \mathrm{mol} \end{aligned} $$ Assume that the reaction takes place under standardstate conditions at \(25^{\circ} \mathrm{C}\).

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 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.)

A piece of silver of mass \(362 \mathrm{~g}\) has a heat capacity of \(85.7 \mathrm{~J} /{ }^{\circ} \mathrm{C}\). What is the specific heat of silver?
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