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Chapter 6: Problem 5

Consider the following statements: "Heat is a form of energy, and energy is conserved. The heat lost by a system must be equal to the amount of heat gained by the surroundings. Therefore, heat is conserved." Indicate everything you think is correct in these statements. Indicate everything you think is incorrect. Correct the incorrect statements and explain.

Short Answer

Expert verified
The correct statements are: 1) Heat is a form of energy, and 2) Energy is conserved. The incorrect statement is: "The heat lost by a system must be equal to the amount of heat gained by the surroundings. Therefore, heat is conserved." The corrected statement should be: "The heat lost by a system must be equal to the amount of heat gained by the surroundings. Therefore, energy is conserved." Heat itself is not conserved, but it can be transformed into other forms of energy, and the total energy of the system is conserved according to the Law of Conservation of Energy.

Step by step solution

01

Identify the correct statements

The following parts of the given statements are correct: 1. "Heat is a form of energy." This is true because heat is defined as the transfer of energy due to a difference in temperature. 2. "Energy is conserved." This is a fundamental principle in physics, known as the Law of Conservation of Energy, which states that energy cannot be created or destroyed, but it can be transformed from one form to another.
02

Identify the incorrect statements

The following part of the given statements is incorrect: 1. "The heat lost by a system must be equal to the amount of heat gained by the surroundings. Therefore, heat is conserved." This statement is not completely false, but it is somewhat misleading.
03

Correct the incorrect statements and explain

We need to rephrase the incorrect statement to avoid confusion: "The heat lost by a system must be equal to the amount of heat gained by the surroundings. Therefore, energy is conserved." The original statement implied that heat is conserved, which might be interpreted as "heat cannot be transformed into other forms of energy," which is not true. Heat can be transformed into other forms of energy, such as mechanical work or electrical energy. As a result, heat itself is not conserved; rather, it is the total energy of the system that is conserved, according to the Law of Conservation of Energy.

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Most popular questions from this chapter

At \(298 \mathrm{~K}\), the standard enthalpies of formation for \(\mathrm{C}_{2} \mathrm{H}_{2}(g)\) and \(\mathrm{C}_{6} \mathrm{H}_{6}(l)\) are \(227 \mathrm{~kJ} / \mathrm{mol}\) and \(49 \mathrm{~kJ} / \mathrm{mol}\), respectively. a. Calculate \(\Delta H^{\circ}\) for $$ \mathrm{C}_{6} \mathrm{H}_{6}(l) \longrightarrow 3 \mathrm{C}_{2} \mathrm{H}_{2}(g) $$ b. Both acetylene \(\left(\mathrm{C}_{2} \mathrm{H}_{2}\right)\) and benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\) can be used as fuels. Which compound would liberate more energy per gram when combusted in air?

Write reactions for which the enthalpy change will be a. \(\Delta H_{\mathrm{f}}^{\circ}\) for solid aluminum oxide. b. The standard enthalpy of combustion of liquid ethanol, \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(l) .\) c. The standard enthalpy of neutralization of sodium hydroxide solution by hydrochloric acid. d. \(\Delta H_{\mathrm{f}}^{\circ}\) for gaseous vinyl chloride, \(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{Cl}(g)\). e. The enthalpy of combustion of liquid benzene, \(\mathrm{C}_{6} \mathrm{H}_{6}(l)\). f. The enthalpy of solution of solid ammonium bromide.

Acetylene \(\left(\mathrm{C}_{2} \mathrm{H}_{2}\right)\) and butane \(\left(\mathrm{C}_{4} \mathrm{H}_{10}\right)\) are gaseous fuels with enthalpies of combustion of \(-49.9 \mathrm{~kJ} / \mathrm{g}\) and \(-49.5 \mathrm{~kJ} / \mathrm{g}\), respectively. Compare the energy available from the combustion of a given volume of acetylene to the combustion energy from the same volume of butane at the same temperature and pressure.

It takes \(585 \mathrm{~J}\) of energy to raise the temperature of \(125.6 \mathrm{~g}\) mercury from \(20.0^{\circ} \mathrm{C}\) to \(53.5^{\circ} \mathrm{C}\). Calculate the specific heat capacity and the molar heat capacity of mercury.

Given the following data $$ \begin{array}{ll} \mathrm{NH}_{3}(g) \longrightarrow \frac{1}{2} \mathrm{~N}_{2}(g)+\frac{3}{2} \mathrm{H}_{2}(g) & \Delta H=46 \mathrm{~kJ} \\ 2 \mathrm{H}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(g) & \Delta H=-484 \mathrm{~kJ} \end{array} $$ calculate \(\Delta H\) for the reaction $$ 2 \mathrm{~N}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(g) \longrightarrow 3 \mathrm{O}_{2}(g)+4 \mathrm{NH}_{3}(g) $$ On the basis of the enthalpy change, is this a useful reaction for the synthesis of ammonia?
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