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Chapter 6: Problem 20

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 bottle with hot water before filling it with hot coffee is a good idea because it pre-warms the bottle, making its inside wall closer in temperature to the hot coffee. This minimizes heat transfer between the coffee and the bottle, allowing the coffee to maintain its temperature for a longer period of time.

Step by step solution

01

Understanding the purpose of using a thermos bottle

A thermos bottle is designed to keep its content (in this case, hot coffee) at a relatively consistent temperature by minimizing heat transfer with the environment. This is achieved by having a double-walled construction and a vacuum between the walls. The vacuum prevents convection and conduction, while the double walls reflect radiant heat back into the bottle.
02

The role of heat transfer in temperature changes

Heat transfer occurs between an object and its surroundings when there is a temperature difference. When a hot liquid (like coffee) is placed in a container (like a thermos), heat will flow from the hot liquid (the coffee) to the surrounding environment (the thermos bottle) until the liquid and the bottle reach a thermal equilibrium.
03

Pre-warming the thermos bottle with hot water

By rinsing the thermos bottle with hot water before filling it with hot coffee, you are pre-warming the bottle. This means that the material of the bottle (the inside wall) is heated up and reaches a temperature closer to that of the hot coffee. This step is crucial in minimizing heat transfer when you eventually pour the hot coffee into the thermos bottle.
04

Benefits of minimizing heat transfer

When you minimize heat transfer from the hot coffee to the thermos bottle, you are helping the coffee maintain its temperature for a longer time. Since the thermos bottle is now closer to the temperature of the coffee due to pre-rinsing it with hot water, the heat loss from the coffee will be less rapid, and the coffee will stay hot for a longer period of time. In conclusion, rinsing your thermos bottle with hot water before filling it with hot coffee is a good idea because it pre-warms the thermos bottle, helps minimize heat transfer, and ultimately maintains the coffee's temperature for a more extended period of time.

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Most popular questions from this chapter

Nitromethane, \(\mathrm{CH}_{3} \mathrm{NO}_{2}\), can be used as a fuel. When the liquid is burned, the (unbalanced) reaction is mainly $$ \mathrm{CH}_{3} \mathrm{NO}_{2}(l)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{N}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g) $$ a. The standard enthalpy change of reaction \(\left(\Delta H_{\mathrm{rxn}}^{\circ}\right)\) for the balanced reaction (with lowest whole- number coefficients) is \(-1288.5 \mathrm{~kJ} .\) Calculate the \(\Delta H_{\mathrm{f}}^{\circ}\) for nitromethane. b. A \(15.0\) - \(\mathrm{L}\) flask containing a sample of nitromethane is filled with \(\mathrm{O}_{2}\) and the flask is heated to \(100 .^{\circ} \mathrm{C}\). At this temperature, and after the reaction is complete, the total pressure of all the gases inside the flask is 950 . torr. If the mole fraction of nitrogen ( \(\chi_{\text {nitrogen }}\) ) is \(0.134\) after the reaction is complete, what mass of nitrogen was produced?

A sample of nickel is heated to \(99.8^{\circ} \mathrm{C}\) and placed in a coffeecup calorimeter containing \(150.0 \mathrm{~g}\) water at \(23.5^{\circ} \mathrm{C}\). After the metal cools, the final temperature of metal and water mixture is \(25.0^{\circ} \mathrm{C}\). If the specific heat capacity of nickel is \(0.444 \mathrm{~J} /{ }^{\circ} \mathrm{C} \cdot \mathrm{g}\), what mass of nickel was originally heated? Assume no heat loss to the surroundings.

The preparation of \(\mathrm{NO}_{2}(g)\) from \(\mathrm{N}_{2}(g)\) and \(\mathrm{O}_{2}(g)\) is an endothermic reaction: $$ \mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{NO}_{2}(g) \text { (unbalanced) } $$ The enthalpy change of reaction for the balanced equation (with lowest whole- number coefficients) is \(\Delta H=67.7 \mathrm{~kJ}\). If \(2.50 \times\) \(10^{2} \mathrm{~mL} \mathrm{~N}_{2}(g)\) at \(100 .{ }^{\circ} \mathrm{C}\) and \(3.50\) atm and \(4.50 \times 10^{2} \mathrm{~mL} \mathrm{O}_{2}(g)\) at \(100 .{ }^{\circ} \mathrm{C}\) and \(3.50 \mathrm{~atm}\) are mixed, what amount of heat is necessary to synthesize the maximum yield of \(\mathrm{NO}_{2}(g)\) ?

A balloon filled with \(39.1\) mol helium has a volume of \(876 \mathrm{~L}\) at \(0.0^{\circ} \mathrm{C}\) and \(1.00\) atm pressure. The temperature of the balloon is increased to \(38.0^{\circ} \mathrm{C}\) as it expands to a volume of \(998 \mathrm{~L}\), the pressure remaining constant. Calculate \(q, w\), and \(\Delta E\) for the helium in the balloon. (The molar heat capacity for helium gas is \(20.8 \mathrm{~J} /{ }^{\circ} \mathrm{C} \cdot\) mol. \()\)

The bomb calorimeter in Exercise 108 is filled with \(987 \mathrm{~g}\) water. The initial temperature of the calorimeter contents is \(23.32^{\circ} \mathrm{C}\). A \(1.056-\mathrm{g}\) sample of benzoic acid \(\left(\Delta E_{\text {comb }}=-26.42 \mathrm{~kJ} / \mathrm{g}\right)\) is combusted in the calorimeter. What is the final temperature of the calorimeter contents?
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