The amount of heat energy required to raise the temperature of $1 \ g$ of helium from $T_1 \ K$ to $T_2 \ K$ at $NTP$ is ........

For a gas,the value of $\frac{R}{C_v} = 0.4$. What is the nature of the gas? ($R$ is the universal gas constant)

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 $J/kg \ K$)?

$A$ gas has $n$ degrees of freedom. The ratio of specific heat of gas at constant volume $(C_v)$ to the specific heat of gas at constant pressure $(C_p)$ will be.

$70 \, cal$ of heat are required to raise the temperature of $2 \, moles$ of an ideal gas at constant pressure from $30^{\circ}C$ to $35^{\circ}C$. The amount of heat required to raise the temperature of the same gas through the same range ($30^{\circ}C$ to $35^{\circ}C$) at constant volume is ..... $cal$ $(R = 2 \, cal/mol \cdot K)$.

$Assertion:$ At a given temperature,the specific heat of a gas at constant pressure $(C_p)$ is always greater than its specific heat at constant volume $(C_v)$.
$Reason:$ When a gas is heated at constant volume,some extra heat is needed compared to that at constant pressure for doing work in expansion.