The values of $C_P$ and $C_V$ for a gas were measured by three different students. The unit is $\text{cal/g mol-K}$. Which set is the most reliable?

For hydrogen gas $C_p - C_v = a$ and for oxygen gas $C_p - C_v = b$. The relation between $a$ and $b$ is given by:

The molar specific heat capacity of a diatomic gas at constant pressure is $C$. The molar specific heat capacity of a monoatomic gas at constant volume is

One mole of an ideal monatomic gas requires $210 \, J$ of heat to raise the temperature by $10 \, K$ when heated at constant pressure. If the same gas is heated at constant volume to raise the temperature by $10 \, K$,then the heat required is ....... $J$.

$c_P$ and $c_V$ are specific heats at constant pressure and constant volume respectively. It is observed that
$c_P - c_V = a$ for hydrogen gas
$c_P - c_V = b$ for nitrogen gas
The correct relation between $a$ and $b$ is

To raise the temperature of a certain mass of gas by $50^{\circ} C$ at a constant pressure,$160$ calories of heat is required. When the same mass of gas is cooled by $100^{\circ} C$ at constant volume,$240$ calories of heat is released. How many degrees of freedom does each molecule of this gas have (assume gas to be ideal)?