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The molar specific heats of an ideal gas at constant pressure and volume are denoted by $C_{P}$ and $C_{V}$ respectively, if $δ = \frac{C_{p}}{C_{v}}$ and R is the universal gas constant, then $C_{V}$ is equal to?

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Rδ-1

δ-1R

δR

1+δ1-δ

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detailed solution

Correct option is A

We know that CP-CV=R but δ=CPCV δCV=Cpsubstitute in above equationδCV-CV=R ⇒CV[δ-1]=R ⇒CV=Rδ-1

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The molar specific heats of an ideal gas at constant pressure and volume are denoted by CP and CV respectively, if δ=CpCv and R is the universal gas constant, then CV is equal to?

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The molar specific heats of an ideal gas at constant pressure and volume are denoted by $C_{P}$ and $C_{V}$ respectively, if $δ = \frac{C_{p}}{C_{v}}$ and R is the universal gas constant, then $C_{V}$ is equal to?