The amount of heat that must be supplied to $35 \ g$ of oxygen at room temperature to raise its temperature by $80^{\circ} C$ at constant volume is (molecular mass of oxygen is $32$ and $R = 8.3 \ J \ mol^{-1} \ K^{-1}$) (in $kJ$)

Given below are observations on molar specific heats at room temperature of some common gases.

Gas	Molar specific heat $(C_v)$ $(cal\, mol^{-1}\, K^{-1})$
Hydrogen	$4.87$
Nitrogen	$4.97$
Oxygen	$5.02$
Nitric oxide	$4.99$
Carbon monoxide	$5.01$
Chlorine	$6.17$

The measured molar specific heats of these gases are markedly different from those for monatomic gases. Typically,molar specific heat of a monatomic gas is $2.92 \; cal/mol\; K$. Explain this difference. What can you infer from the somewhat larger (than the rest) value for chlorine?

$176 \text{ grams}$ of $CO_2$ can change its temperature from $0^{\circ} C$ to $30^{\circ} C$ by absorbing $3600 \text{ joules}$ of thermal energy. The molar specific heat of $CO_2$ in $J \ mol^{-1} K^{-1}$ is:

The specific heat of helium at constant volume is $12.6 \ J \ mol^{-1} \ K^{-1}$. The specific heat of helium at constant pressure in $J \ mol^{-1} \ K^{-1}$ is about (Assume the temperature of the gas is moderate,universal gas constant,$R=8.314 \ J \ mol^{-1} \ K^{-1}$)

For a gas,the difference between the two specific heats is $4150 \ J/kg \ K$. What is the specific heat at constant volume of the gas if the ratio of specific heats is $1.4$ (in $J/kg \ K$)?

Match the following ( $f$ is number of degrees of freedom):

	Gases		$C_P/C_V$ value
$A$	Monoatomic	$I$	$(4+f)/(3+f)$
$B$	Diatomic (rigid)	$II$	$5/3$
$C$	Diatomic (non-rigid)	$III$	$7/5$
$D$	Polyatomic	$IV$	$9/7$