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(B) $1$. According to Mayer's relation,$C_p - C_v = R$,where $R$ is the universal gas constant. This value is independent of the atomicity of the gas.

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$C_p + C_v$ is larger for a diatomic ideal gas than for a monoatomic ideal gas

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(B) $1$. According to Mayer's relation,$C_p - C_v = R$,where $R$ is the universal gas constant. This value is independent of the atomicity of the gas.$2$. The ratio $\gamma = C_p/C_v$ is given by $1 + 2/f$,where $f$ is the degree of freedom. For monoatomic gas $(f=3)$,$\gamma = 1.67$. For diatomic gas $(f=5)$,$\gamma = 1.4$. Thus,$\gamma$ decreases as atomicity increases.$3$. The sum $C_p + C_v$ can be expressed as $C_v(1 + \gamma)$. Since $C_v = fR/2$,we have $C_p + C_v = (fR/2)(1 + 1 + 2/f) = (fR/2)(2 + 2/f) = R(f + 1)$.$4$. For monoatomic gas $(f=3)$,$C_p + C_v = 4R$. For diatomic gas $(f=5)$,$C_p + C_v = 6R$. Therefore,$C_p + C_v$ is larger for a diatomic ideal gas.

$C_v$ and $C_p$ denote the molar specific heat capacities of a gas at constant volume and constant pressure,respectively. Then

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