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Chapter 6: Problem 25

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 a thermos bottle with hot water before filling it with hot coffee is a good idea because it preheats the inner wall of the thermos, minimizing the temperature difference and reducing heat transfer between the coffee and the thermos. This helps maintain the coffee's temperature and allows it to remain hot for a longer period.

Step by step solution

01

Understanding Thermos and Insulation Properties

A thermos bottle is designed to maintain the temperature of its contents, either hot or cold, by providing an insulating barrier between the contents and the outside environment. The insulation properties of a thermos bottle come from the vacuum and reflective layer between the inner and outer walls, which prevents heat transfer through conduction, convection, and radiation.
02

Heat Transfer

When filling a thermos bottle with hot coffee, the heat energy in the coffee primarily transfers to the inner wall of the thermos, causing the inner wall to heat up. This process will eventually reach a state of equilibrium where the heat loss from the coffee to the thermos' inner wall will be minimal, allowing the coffee to remain hot for an extended period.
03

Preheating the Thermos Bottle

Rinsing the thermos bottle with hot water before filling it with hot coffee preheats the inner wall of the thermos. This process helps minimize the temperature difference between the thermos' inner wall and the hot coffee, reducing the amount of heat transferred from the coffee to the thermos when it is poured in.
04

Reducing Heat Loss

By minimizing the initial heat transfer between the hot coffee and the thermos bottle, the coffee's temperature will remain more consistent and hot for a longer period. This means that the coffee's heat energy is being used to maintain its temperature instead of losing it to the thermos' inner wall during the initial filling process. In conclusion, rinsing a thermos bottle with hot water before filling it with hot coffee is a good idea because it preheats the inner wall of the thermos, reducing heat loss from the coffee to the thermos. This helps to maintain the coffee's temperature, allowing it to remain hot for a longer period.

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Most popular questions from this chapter

Calculate \(\Delta E\) for each of the following. a. \(q=-47 \mathrm{kJ}, w=+88 \mathrm{kJ}\) b. \(q=+82 \mathrm{kJ}, w=-47 \mathrm{kJ}\) c. \(q=+47 \mathrm{kJ}, w=0\) d. In which of these cases do the surroundings do work on the system?

Given the following data $$ \begin{aligned} \mathrm{P}_{4}(s)+6 \mathrm{Cl}_{2}(g) \longrightarrow 4 \mathrm{PCl}_{3}(g) & \Delta H=-1225.6 \mathrm{kJ} \\ \mathrm{P}_{4}(s)+5 \mathrm{O}_{2}(g) \longrightarrow \mathrm{P}_{4} \mathrm{O}_{10}(s) & \Delta H=-2967.3 \mathrm{kJ} \end{aligned} $$ $$ \begin{array}{cc}{\mathrm{PCl}_{3}(g)+\mathrm{Cl}_{2}(g) \longrightarrow \mathrm{PCl}_{5}(g)} & {\Delta H=-84.2 \mathrm{kJ}} \\\ {\mathrm{PCl}_{3}(g)+\frac{1}{2} \mathrm{O}_{2}(g) \longrightarrow \mathrm{Cl}_{3} \mathrm{PO}(g)} & {\Delta H=-285.7 \mathrm{kJ}}\end{array} $$ calculate \(\Delta H\) for the reaction $$ \mathrm{P}_{4} \mathrm{O}_{10}(s)+6 \mathrm{PCl}_{5}(g) \longrightarrow 10 \mathrm{Cl}_{3} \mathrm{PO}(g) $$

Consider a balloon filled with helium at the following conditions. $$ \begin{array}{l}{313 \mathrm{g} \mathrm{He}} \\ {1.00 \mathrm{atm}} \\ {1910 . \mathrm{L}} \\ {\text { Molar Heat Capacity }=20.8 \mathrm{J} / \mathrm{C} \cdot \mathrm{mol}}\end{array} $$ The temperature of this balloon is decreased by \(41.6^{\circ} \mathrm{C}\) as the volume decreases to \(1643 \mathrm{L},\) with the pressure remaining constant. Determine \(q, w,\) and $\Delta E(\text { in } \mathrm{kJ} \text { ) for the compression of }$ the balloon.

Assume that \(4.19 \times 10^{6} \mathrm{kJ}\) of energy is needed to heat a home. If this energy is derived from the combustion of methane \(\left(\mathrm{CH}_{4}\right),\) what volume of methane, measured at STP, must be burned? $\left(\Delta H_{\text { combustion }}^{\circ} \text { for } \mathrm{CH}_{4}=-891 \mathrm{kJ} / \mathrm{mol}\right)$

A gas absorbs 45 kJ of heat and does 29 kJ of work. Calculate \(\Delta E .\)
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