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Chapter 6: Problem 142

Give an example for each of the following situations: (a) Adding heat to a system raises its temperature, (b) adding heat to a system does not change (raise) its temperature, and (c) a system's temperature is changed even though no heat is added or removed from it.

Short Answer

Expert verified
Situation A: Heating a pot of water on a stovetop. Situation B: Melting ice at 0°C. Situation C: The temperature rise in air as it is compressed in a bicycle pump.

Step by step solution

01

Situation (a)

In a situation where the addition of heat raises the system's temperature, we can choose a pot of water at room temperature. When we place the pot on a stovetop and turn the heat on, heat energy will be transferred from the stove to the pot, resulting in an increase in water temperature.
02

Situation (b)

An example where the addition of heat does not raise the system's temperature could be a melting ice cube. If we take ice at 0°C and add heat to it, the state of water changes from solid to liquid during this phase change. But the temperature remains the same until all the ice has melted. This process is due to the heat being used to break the bonds holding the molecules together in a solid state instead of raising the temperature.
03

Situation (c)

In situations where temperature changes even though no heat is added or removed, such alteration is possible by doing work on the system. A good example is a bicycle pump. As you pump air into a tire, the air being compressed - work being done on it - increases its temperature even though no heat was added.

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Most popular questions from this chapter

Why is it dangerous to add water to a concentrated acid such as sulfuric acid in a dilution process?

Why is the lattice energy of a solid always a positive quantity? Why is the hydration of ions always a negative quantity?

Which is the more negative quantity at \(25^{\circ} \mathrm{C}: \Delta H_{\mathrm{f}}^{\circ}\) for \(\mathrm{H}_{2} \mathrm{O}(l)\) or \(\Delta H_{\mathrm{f}}^{\circ}\) for \(\mathrm{H}_{2} \mathrm{O}(g) ?\)

Given the thermochemical equations: $$\begin{array}{c}\mathrm{Br}_{2}(l)+\mathrm{F}_{2}(g) \longrightarrow 2 \mathrm{BrF}(g) \\ \Delta H^{\circ}=-188 \mathrm{~kJ} / \mathrm{mol} \\ \mathrm{Br}_{2}(l)+3 \mathrm{~F}_{2}(g) \longrightarrow 2 \mathrm{BrF}_{3}(g) \\\ \Delta H^{\circ}=-768 \mathrm{~kJ} / \mathrm{mol}\end{array} $$calculate the \(\Delta H_{\mathrm{rxn}}^{\circ}\) for the reaction$$\operatorname{BrF}(g)+\mathrm{F}_{2}(g) \longrightarrow \operatorname{BrF}_{3}(g)$$

For which of the following reactions does \(\Delta H_{\mathrm{rxn}}^{\circ}=\) \(\Delta H_{\mathrm{f}}^{\circ} ?\) (a) \(\mathrm{H}_{2}(g)+\mathrm{S}(\) rhombic \() \longrightarrow \mathrm{H}_{2} \mathrm{~S}(g)\) (b) C(diamond) \(+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)\) (c) \(\mathrm{H}_{2}(g)+\mathrm{CuO}(s) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{Cu}(s)\) (d) \(\mathrm{O}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{O}_{3}(g)\)
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