(C) Given,at constant pressure heat $Q_p = 306 \ J$.Number of moles,$n = 2$.Change in temperature,$\Delta T = 35 - 25 = 10 \ K$.We know that $Q_p = n

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(C) Given,at constant pressure heat $Q_p = 306 \ J$.Number of moles,$n = 2$.Change in temperature,$\Delta T = 35 - 25 = 10 \ K$.We know that $Q_p = n C_p \Delta T$.Substituting the values: $306 = 2 \times C_p \times 10$.Thus,$C_p = \frac{306}{20} = 15.3 \ J \ mol^{-1} K^{-1}$.According to Mayer's relation,$C_p - C_V = R$.Using $R \approx 8.314 \ J \ mol^{-1} K^{-1}$,we get $C_V = 15.3 - 8.314 = 6.986 \ J \ mol^{-1} K^{-1}$.The heat required at constant volume is $Q_V = n C_V \Delta T$.$Q_V = 2 \times 6.986 \times 10 = 139.72 \ J \approx 140 \ J$.

Class 11 Physics Kinetic Theory of Gases Molar Specific Heat of gas and relation between them (Mayer's formula)

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$306 \ J$ of heat is required to raise the temperature of $2 \ moles$ of an ideal gas at constant pressure from $25^{\circ} C$ to $35^{\circ} C$. The amount of heat required to raise the temperature of the same gas through the same range at constant volume is (in $J$)

AP EAMCET 2020 All AP EAMCET

A
$306$
B
$153$
C
$140$
D
$80$

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Kinetic Theory of Gases

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Molar Specific Heat of gas and relation between them (Mayer's formula)

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$306 \ J$ of heat is required to raise the temperature of $2 \ moles$ of an ideal gas at constant pressure from $25^{\circ} C$ to $35^{\circ} C$. The amount of heat required to raise the temperature of the same gas through the same range at constant volume is (in $J$)

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