Show that the volume expansion coefficient of an ideal gas is \(\beta=1 / T\), where \(T\) is the absolute temperature.

Short Answer

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Question: Show that the volume expansion coefficient of an ideal gas is inversely proportional to the absolute temperature. Answer: The volume expansion coefficient (β) of an ideal gas is inversely proportional to the absolute temperature, which means β = 1 / T.

Step by step solution

01

Understand the volume expansion coefficient and ideal gas law

The volume expansion coefficient (β) of a substance is a measure of how the volume of the substance changes with temperature, at a constant pressure. Mathematically, it is defined as: \(\beta = \frac{1}{V} \frac{\partial V}{\partial T}\Big|_P\) where V is the volume, T is the absolute temperature, and P is the pressure. The ideal gas law relates the pressure (P), volume (V), and temperature (T) of an ideal gas: \(PV = nRT\) where n is the number of moles of the gas and R is the ideal gas constant.
02

Express the volume as a function of temperature and pressure

From the ideal gas law, we can express the volume (V) as a function of temperature (T) and pressure (P): \(V = \frac{nRT}{P}\)
03

Calculate the partial derivative of the volume with respect to the temperature

Now, we will calculate the partial derivative of the volume with respect to the temperature (keeping the pressure constant): \(\frac{\partial V}{\partial T}\Big|_P = \frac{\partial}{\partial T} \left(\frac{nRT}{P}\right)\Big|_P = \frac{nR}{P}\) Here, we treat n, R, and P as constants.
04

Calculate the volume expansion coefficient

Finally, we will plug our expression for the partial derivative of the volume with respect to the temperature back into the equation for the volume expansion coefficient: \(\beta = \frac{1}{V} \frac{\partial V}{\partial T}\Big|_P = \frac{1}{\frac{nRT}{P}} \frac{nR}{P}\) Simplifying, we get: \(\beta = \frac{1}{T}\) Therefore, the volume expansion coefficient of an ideal gas is inversely proportional to the absolute temperature, β = 1 / T.

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Most popular questions from this chapter

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