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Chapter 8: Problem 1086

The temperature of a substance increases by \(27^{\circ} \mathrm{C}\) What is the value of this increase of Kelvin scale? (A) \(300 \mathrm{~K}\) (B) \(2-46 \mathrm{~K}\) (C) \(7 \mathrm{~K}\) (D) \(27 \mathrm{~K}\)

Short Answer

Expert verified
The value of the temperature increase on the Kelvin scale is \(27 \mathrm{~K}\).

Step by step solution

01

Understand the relationship between Celsius and Kelvin scales

The Celsius and Kelvin scales have the same interval or "size" between their degrees. The difference between them is that the Kelvin scale starts at absolute zero (-273.15°C), while the Celsius scale starts at the freezing point of water (0°C).
02

Convert the temperature increase from Celsius to Kelvin

Since both Celsius and Kelvin scales have the same interval, a temperature change of 27°C is equal to a temperature change of 27K.
03

Identify the correct answer

Comparing our result with the given options, we can see that the correct answer is: (D) \(27 \mathrm{~K}\)

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Most popular questions from this chapter

If du represents the increase in internal energy of a thermodynamic system and dw the work done by the system, which of the following statement is true? (A) \(\mathrm{du}=\mathrm{dw}\) in isothermal process (C) \(\mathrm{du}=-\mathrm{dw}\) in an aidabatic process (B) \(\mathrm{du}=\mathrm{dw}\) in aidabatic process (D) \(\mathrm{du}=-\mathrm{dw}\) in an isothermal process

The isothermal Bulk modulus of an ideal gas at pressure \(\mathrm{P}\) is (A) \(\mathrm{vP}\) (B) \(\mathrm{P}\) (C) \((\mathrm{p} / 2)\) (D) \((\mathrm{p} / \mathrm{v})\)

If a quantity of heat \(1163.4 \mathrm{~J}\) is supplied to one mole of nitrogen gas, at room temperature at constant pressure, then the rise in temperature is \(\mathrm{R}=8.31\\{\mathrm{~J} /(\mathrm{m} \cdot 1 . \mathrm{k})\\}\) (A) \(28 \mathrm{~K}\) (B) \(65 \mathrm{~K}\) (C) \(54 \mathrm{~K}\) (D) \(40 \mathrm{~K}\)

The Volume of air increases by \(5 \%\) in an adiabatic expansion. The percentage decrease in its Pressure will be (A) \(5 \%\) (B) \(6 \%\) (C) \(7 \%\) (D) \(8 \%\)

The Volume of an ideal gas is 1 liter column and its Pressure is equal to $72 \mathrm{~cm}\( of \)\mathrm{Hg}$. The Volume of gas is made 900 \(\mathrm{cm}^{3}\) by compressing it isothermally. The stress of the gas will be \(\ldots \ldots \ldots \ldots .\) Hg column. (A) \(4 \mathrm{~cm}\) (B) \(6 \mathrm{~cm}\) (C) \(7 \mathrm{~cm}\) (D) \(8 \mathrm{~cm}\)
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