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Chapter 6: Problem 2

What is heat? How does heat differ from thermal energy? Under what condition is heat transferred from one system to another?

Short Answer

Expert verified
Heat is energy transferred from a hotter object to a cooler one due to a temperature difference, while thermal energy is the total kinetic and potential energy of an object's particles. Heat is transferred from one system to another when there's a temperature difference between them, with the transfer continuing until the two systems reach thermal equilibrium.

Step by step solution

01

Define Heat

Heat is a form of energy that is transferred from a hotter object to a cooler one. It is always transferred due to a temperature difference and tends to equalize the temperature difference.
02

Define Thermal Energy

Thermal energy is the total kinetic (motion-based) and potential energy of the particles in an object. It corresponds to how much movement and vibration the particles of the object have.
03

Distinguish Between Heat and Thermal Energy

Although both are forms of energy, heat and thermal energy are distinct from each other. Thermal energy is dependent on the temperature, mass, and type of object, while heat is the transfer of this energy from a warmer object to a cooler one.
04

Identify Conditions for Heat Transfer

Heat is transferred from one system to another until the two systems arrive at the same temperature, a condition known as thermal equilibrium. The transfer occurs from the system with higher temperature to the one with lower temperature. It can occur through one of three mechanisms - conduction, convection, or radiation - depending on the nature of the systems involved.

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Most popular questions from this chapter

The standard enthalpy change \(\Delta H^{\circ}\) for the thermal decomposition of silver nitrate according to the following equation is \(+78.67 \mathrm{~kJ}\) : $$ \mathrm{AgNO}_{3}(s) \longrightarrow \mathrm{AgNO}_{2}(s)+\frac{1}{2} \mathrm{O}_{2}(g) $$ The standard enthalpy of formation of \(\mathrm{AgNO}_{3}(s)\) is \(-123.02 \mathrm{~kJ} / \mathrm{mol}\). Calculate the standard enthalpy of formation of \(\mathrm{AgNO}_{2}(s)\).

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.

The standard enthalpy change for the following reaction is \(436.4 \mathrm{~kJ} / \mathrm{mol}\) : $$ \mathrm{H}_{2}(g) \longrightarrow \mathrm{H}(g)+\mathrm{H}(g) $$ Calculate the standard enthalpy of formation of atomic hydrogen (H).

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?

A quantity of \(2.00 \times 10^{2} \mathrm{~mL}\) of \(0.862 \mathrm{M} \mathrm{HCl}\) is mixed with \(2.00 \times 10^{2} \mathrm{~mL}\) of \(0.431 \mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}\) in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of the \(\mathrm{HCl}\) and \(\mathrm{Ba}(\mathrm{OH})_{2}\) solutions is the same at \(20.48^{\circ} \mathrm{C}\). For the process $$ \mathrm{H}^{+}(a q)+\mathrm{OH}^{-}(a q) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l) $$ the heat of neutralization is \(-56.2 \mathrm{~kJ} / \mathrm{mol}\). What is the final temperature of the mixed solution?
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