Medium
One mole of an ideal gas requires $207 \, J$ 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 the same $10 \, K$,the heat required is ...... $J$ (Given the gas constant $R = 8.3 \, J/mol \cdot K$)
- A$198.7$
- B$29$
- C$215.3$
- D$124$
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If $C_{p}$ and $C_{v}$ are molar specific heats of an ideal gas at constant pressure and volume respectively and $\gamma$ is $C_{p} / C_{v}$,then $C_{p} =$ (where $R$ is the universal gas constant).
The molar specific heats of an ideal gas at constant pressure and volume are denoted by $C_{P}$ and $C_{V}$ respectively. If $\gamma = \frac{C_{P}}{C_{V}}$ and $R$ is the universal gas constant,then $C_{V}$ is equal to
An ideal mono-atomic gas is taken through a process such that $dQ = 3dU$. The molar heat capacity for this process is: (in $R$)
Medium
View SolutionWhich one of the following is $NOT$ a correct expression for an ideal gas?
[$C_{P}=$ Molar specific heat of a gas at constant pressure,
$C_{V}=$ Molar specific heat of a gas at constant volume,
$\gamma=$ Ratio of two specific heats of a gas,$R=$ Universal gas constant]
[$C_{P}=$ Molar specific heat of a gas at constant pressure,
$C_{V}=$ Molar specific heat of a gas at constant volume,
$\gamma=$ Ratio of two specific heats of a gas,$R=$ Universal gas constant]
When an ideal diatomic gas is heated at constant pressure,the fraction of the heat utilized to increase the internal energy of the gas is
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