Find the ratio of specific heat at constant pressure $(C_p)$ to the specific heat at constant volume $(C_v)$ for $NH_3$.

The molar specific heat at constant pressure of an ideal gas is $(7/2)R$. The ratio of specific heat at constant pressure to that at constant volume is

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

$A$ cylinder with fixed capacity of $67.2 \, L$ contains helium gas at $STP$. The amount of heat needed to raise the temperature of the gas by $20 \, ^oC$ is ..... $J$ [Given that $R = 8.31 \, J \, mol^{-1} \, K^{-1}$]

$70 \, cal$ 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 ..... $cal$ $(R = 2 \, cal/mol \cdot K)$.

$1 \, mole$ of a gas requires $40 \, calories$ of heat to raise its temperature from $20^{\circ}C$ to $30^{\circ}C$ at constant pressure. How many calories of heat are required to raise the temperature of the same gas by the same amount at constant volume? $(R = 2 \, cal \, mol^{-1} K^{-1})$