For hydrogen gas,$C_P - C_V = a$,and for oxygen gas,$C_P - C_V = b$. The relationship between $a$ and $b$ is given by: (where $C_P$ and $C_V$ are molar specific heats at constant pressure and constant volume,respectively.)

  • A
    $a = 16b$
  • B
    $b = 16a$
  • C
    $a = 4b$
  • D
    $a = b$

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What is the correct relationship between molar specific heat at constant pressure $(C_P)$ and constant volume $(C_V)$? ($R$ is the universal gas constant)

The ratio of the specific heats $\frac{C_{p}}{C_{v}}=\gamma$ in terms of degrees of freedom $n$ is given by

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What is the significance of the heat capacity ratio $\gamma = \frac{C_{P}}{C_{V}}$ for a gas?

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What amount of heat (in $J$) must be supplied to $2.0 \times 10^{-2} \; kg$ of nitrogen (at room temperature) to raise its temperature by $45 \; ^{\circ}C$ at constant pressure? (Molecular mass of $N_{2} = 28; R = 8.3 \; J \; mol^{-1} K^{-1}$.)

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