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Chapter 30: Problem 2834

Amount of heat required to raise the temperature of a body through $1 \mathrm{k}$ is called its (A) water equivalent (B) Thermal capacity (C) entropy (D) specific heat

Short Answer

Expert verified
The correct term is (B) Thermal capacity, as it refers to the amount of heat required to raise the temperature of a body through 1 Kelvin.

Step by step solution

01

Define water equivalent

Water equivalent is the amount of water that can be heated with the same amount of heat as the given body and exhibit the same change in temperature.
02

Define thermal capacity

Thermal capacity is the amount of heat required to raise the temperature of a body by 1 Kelvin. It is equal to the mass of the body times its specific heat capacity.
03

Define entropy

Entropy is a measure of the disorder of a system, or the amount of energy unavailable to do work.
04

Define specific heat

Specific heat is the amount of heat required to raise the temperature of a unit mass of a substance by 1 Kelvin.
05

Determine the correct term

Based on the definitions, the correct term is (B) Thermal capacity, which is the amount of heat required to raise the temperature of a body through 1 Kelvin.

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Most popular questions from this chapter

\(100 \mathrm{~g}\) ice at \(0^{\circ} \mathrm{C}\) placed in \(100 \mathrm{~g}\) water at \(100^{\circ} \mathrm{C}\). The final temperature of the mixture will be........ (Latent heat of ice is \(80 \mathrm{Cal} / \mathrm{g}\), and specific heat of water is \(1 \mathrm{Cal} / \mathrm{g} \mathrm{C}^{\circ}\) ) (A) \(10^{\circ} \mathrm{C}\) (B) \(20^{\circ} \mathrm{C}\) (C) \(30^{\circ} \mathrm{C}\) (D) \(50^{\circ} \mathrm{C}\)

Two liquids of equal volume are thoroughly mixed. If their specific heat are \(c_{1}, c_{2}\), temperatures \(\theta_{1}, \theta_{2}\) and densities \(\mathrm{d}_{1}, \mathrm{~d}_{2}\) respectively. What is the final temperature of the mixture ? (A) $\left\\{\left(\mathrm{d}_{1} \mathrm{c}_{1} \theta_{1}+\mathrm{d}_{2} \mathrm{c}_{2} \theta_{2}\right) /\left(\mathrm{d}_{1} \theta_{1}+\mathrm{d}_{2} \theta_{2}\right)\right\\}$ (B) $\left\\{\left(\mathrm{c}_{1} \theta_{1}+\mathrm{c}_{2} \theta_{2}\right) /\left(\mathrm{d}_{1} \mathrm{c}_{1}+\mathrm{d}_{2} \mathrm{c}_{2}\right)\right\\}$ (C) $\left\\{\left(\mathrm{d}_{1} \theta_{1}+\mathrm{d}_{2} \theta_{2}\right) /\left(\mathrm{c}_{1} \theta_{1}+\mathrm{c}_{2} \theta_{2}\right)\right\\}$ (D) $\left\\{\left(\mathrm{d}_{1} \mathrm{c}_{1} \theta_{1}+\mathrm{d}_{2} \mathrm{c}_{2} \theta_{2}\right) /\left(\mathrm{d}_{1} \mathrm{c}_{1}+\mathrm{d}_{2} \mathrm{c}_{2}\right)\right\\}$

A centigrade and a Fahrenheit thermometer one dipped in boiling water. The water temperature is lowered until the Fahrenheit thermometer registers \(140^{\circ}\). What is the fall in temperatures as registered by the centigrade thermometer? (A) \(30^{\circ}\) (B) \(40^{\circ}\) (C) \(60^{\circ}\) (D) \(80^{\circ}\)

The temperature of equal masses of three different liquids \(\mathrm{X}\), \(\mathrm{Y}, \mathrm{Z}\) are \(12^{\circ} \mathrm{C}, 19^{\circ} \mathrm{C}\) and \(28^{\circ} \mathrm{C}\) respectively. The temperature when \(\mathrm{X}\) and \(\mathrm{Y}\) are mixed is \(16^{\circ} \mathrm{C}\) and when \(\mathrm{Y}\) and \(\mathrm{Z}\) are mixed is \(23^{\circ} \mathrm{C}\) what is the temperature when \(\mathrm{X}\) and \(\mathrm{Z}\) are mixed ? (A) \(21.6^{\circ} \mathrm{C}\) (B) \(18.5^{\circ} \mathrm{C}\) (C) \(23.25^{\circ} \mathrm{C}\) (D) \(20.3^{\circ} \mathrm{C}\)
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