Class 11PhysicsKinetic Theory of GasesMolar Specific Heat of gas and relation between them (Mayer's formula)
Difficult$70 \, cal$ 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 ..... $cal$ $(R = 2 \, cal/mol \cdot K)$.
- A$30$
- B$50$
- C$70$
- D$90$
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Which 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]
$A$ triatomic,diatomic,and monatomic gas are supplied the same amount of heat at constant pressure. Then:
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View SolutionThe 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 $kJ$)
When $40 \ J$ of heat is absorbed by a monatomic gas,the increase in the internal energy of the gas is (in $J$)
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