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Chapter 7: Problem 21

Why is it a good idea to rinse your thermos bottle with hot water before filling it with hot coffee?

Short Answer

Expert verified
Rinsing your thermos with hot water before filling it with hot coffee is a good idea because it preheats the thermos, reducing heat transfer between the thermos and the coffee. This helps to maintain the ideal temperature of the coffee for a longer duration, preserving its taste and quality, and providing a more enjoyable drinking experience.

Step by step solution

01

Understand the Purpose of a Thermos

A thermos is designed to keep its contents (such as hot coffee) at a relatively constant temperature for an extended period. It works by having two walls with a vacuum between them. This vacuum prevents heat transfer through conduction and convection, thus retaining the temperature of the contents inside.
02

Importance of Heat Retention

Keeping the coffee at a relatively constant temperature is crucial for several reasons. First, it preserves the taste and quality of the coffee. Second, it ensures the coffee stays hot for a more extended period, making it more enjoyable to drink. Finally, it can prevent burns or other accidents from handling a hot container.
03

Heat Transfer Principles

Three methods of heat transfer are conduction, convection, and radiation. In our case, both conduction and convection play a role in affecting the temperature of the contents inside the thermos. Conduction occurs when two objects with different temperatures touch each other, while convection happens as a fluid (in this case, air) rises when heated due to density differences.
04

Initial Temperature of the Thermos

When a thermos is at room temperature, the air inside is cooler than the hot coffee you plan to pour into it. The cold air inside the thermos will absorb some of the heat from the coffee, thus cooling it down faster than desired.
05

Rinsing the Thermos with Hot Water

By rinsing the thermos with hot water before filling it with hot coffee, you are preheating the thermos and eliminating the cool air that would absorb the heat from the coffee. When you pour the hot coffee into the preheated thermos, there is much less of a temperature difference between the thermos and the coffee. As a result, it reduces the amount of heat transfer and maintains the coffee's temperature for a longer duration.
06

Conclusion

It's a good idea to rinse your thermos with hot water before filling it with hot coffee, as it preheats the thermos, reduces heat transfer, and maintains the ideal temperature of the coffee for a more extended period. This process preserves the taste and quality of the coffee and provides an enjoyable drinking experience.

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Most popular questions from this chapter

Assuming gasoline is pure \(\mathrm{C}_{8} \mathrm{H}_{18}(l),\) predict the signs of \(q\) and \(w\) for the process of combusting gasoline into \(\mathrm{CO}_{2}(g)\) and \(\mathrm{H}_{2} \mathrm{O}(g)\).

The standard enthalpy of combustion of ethene gas, \(\mathrm{C}_{2} \mathrm{H}_{4}(g)\) is \(-1411.1 \mathrm{kJ} / \mathrm{mol}\) at \(298 \mathrm{K}\). Given the following enthalpies of formation, calculate \(\Delta H_{\mathrm{f}}^{\circ}\) for \(\mathrm{C}_{2} \mathrm{H}_{4}(g)\). $$\begin{array}{ll}\mathrm{CO}_{2}(g) & -393.5 \mathrm{kJ} / \mathrm{mol} \\\\\mathrm{H}_{2} \mathrm{O}(l) & -285.8 \mathrm{kJ} / \mathrm{mol}\end{array}$$

Consider 2.00 moles of an ideal gas that are taken from state \(A\) \(\left(P_{A}=2.00 \mathrm{atm}, V_{A}=10.0 \mathrm{L}\right)\) to state \(B\left(P_{B}=1.00 \mathrm{atm}, V_{B}=\right.\) \(30.0 \mathrm{L})\) by two different pathways: These pathways are summarized on the following graph of \(P\) versus \(V:\) Calculate the work (in units of J) associated with the two pathways. Is work a state function? Explain.

For the reaction \(\mathrm{HgO}(s) \rightarrow \mathrm{Hg}(l)+\frac{1}{2} \mathrm{O}_{2}(g), \Delta H=+90.7 \mathrm{kJ}\). a. What quantity of heat is required to produce 1 mole of mercury by this reaction? b. What quantity of heat is required to produce 1 mole of oxygen gas by this reaction? c. What quantity of heat would be released in the following reaction as written? $$2 \mathrm{Hg}(l)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{HgO}(s)$$

Given the following data $$\begin{array}{ll}\mathrm{Fe}_{2} \mathrm{O}_{3}(s)+3 \mathrm{CO}(g) \longrightarrow 2 \mathrm{Fe}(s)+3 \mathrm{CO}_{2}(g) & \Delta H^{\circ}=-23 \mathrm{kJ} \\ 3 \mathrm{Fe}_{2} \mathrm{O}_{3}(s)+\mathrm{CO}(g) \longrightarrow 2 \mathrm{Fe}_{3} \mathrm{O}_{4}(s)+\mathrm{CO}_{2}(g) & \Delta H^{\circ}=-39 \mathrm{kJ} \\ \mathrm{Fe}_{3} \mathrm{O}_{4}(s)+\mathrm{CO}(g) \longrightarrow 3 \mathrm{FeO}(s)+\mathrm{CO}_{2}(g) & \Delta H^{\circ}=18 \mathrm{kJ} \end{array}$$ calculate \(\Delta H^{\circ}\) for the reaction $$\mathrm{FeO}(s)+\mathrm{CO}(g) \longrightarrow \mathrm{Fe}(s)+\mathrm{CO}_{2}(g)$$
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