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(B) At constant pressure,the heat required is given by $Q_p = n C_p \Delta T$.Given $n = 2 \ moles$,$\Delta T = 35^{\circ} C - 25^{\circ} C = 10 \ K$,

Vedclass · Accepted Answer

$144$

Vedclass · Answer

(B) At constant pressure,the heat required is given by $Q_p = n C_p \Delta T$.Given $n = 2 \ moles$,$\Delta T = 35^{\circ} C - 25^{\circ} C = 10 \ K$,and $Q_p = 310 \ J$.$310 = 2 	imes C_p 	imes 10 \Rightarrow C_p = \frac{310}{20} = 15.5 \ J \ mol^{-1} K^{-1}$.Using the relation $C_p - C_V = R$,where $R \approx 8.3 \ J \ mol^{-1} K^{-1}$:$C_V = C_p - R = 15.5 - 8.3 = 7.2 \ J \ mol^{-1} K^{-1}$.At constant volume,the heat required is $Q_V = n C_V \Delta T$.$Q_V = 2 	imes 7.2 	imes 10 = 144 \ J$.

$310 \ J$ 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 gas through the same range at constant volume is (in $J$)

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