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A 2.00-mol sample of a diatomic ideal gas expands slowly and adiabatically from a pressure of 5.00 atm5.00 \mathrm{~atm} and a volume of 12.0 L12.0 \mathrm{~L} to a final volume of 30.0 L30.0 \mathrm{~L}. What are the initial and final temperatures?

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Concepts and Principles

  • When an ideal gas undergoes a slow adiabatic volume change (Q=0\textcolor{#c34632}{Q=0}), its pressure and volume are related by:

PVγ=constant\begin{equation*} PV^{\gamma}=\text{constant}\tag{1} \end{equation*}

Where γ=CP/CV\textcolor{#c34632}{\gamma=C_P/C_V} is the ratio of molar specific heats for the gas. For a diatomic gas, γ=1.4\textcolor{#c34632}{\gamma=1.4}.

  • Equation of State of an Ideal Gas: an ideal gas is one for which the pressure P\textcolor{#c34632}{P}, volume V\textcolor{#c34632}{V}, and temperature T\textcolor{#c34632}{T} are related by:

PV=nRT\begin{equation*} PV=nRT\tag{1} \end{equation*}

Where,

n\textcolor{#c34632}{n} is the number of moles of the gas present.
R\textcolor{#c34632}{R} is the universal gas constant and has a value 8.314  J/molK\textcolor{#c34632}{8.314\;\mathrm{J/mol\cdot K}}.

  • The change in the internal energy of n\textcolor{#c34632}{n} moles of a confined ideal gas that undergoes a temperature change ΔT\textcolor{#c34632}{\Delta T} due to any process is:

ΔEint=nCVΔT\begin{equation*} \Delta E_{\text{int}}=nC_V\Delta T\tag{3} \end{equation*}

Where CV\textcolor{#c34632}{C_V} is the molar specific heat at constant volume for the gas.

  • First Law of Thermodynamics: it is the principle of conservation of energy for a thermodynamic process which is expressed as:

ΔEint=Q+W\begin{equation*} \Delta E_{\text{int}}=Q+W\tag{4} \end{equation*}

Where ΔEint\textcolor{#c34632}{\Delta E_{\text{int}}} is the internal energy of the system, Q\textcolor{#c34632}{Q} is the energy transferred into the system by heat between the system and its surroundings, and W\textcolor{#c34632}{W} is the work done on the system.

In this problem, I am displaying rounded intermediate values for practical purposes. However, calculations are made using the unrounded values.

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