Consider the following volume-temperature (V- | vedclass

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(D) For an ideal gas,the change in enthalpy $(\Delta H)$ depends only on the initial and final temperatures,as enthalpy is a state function.Given:Numb

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$8120$

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(D) For an ideal gas,the change in enthalpy $(\Delta H)$ depends only on the initial and final temperatures,as enthalpy is a state function.Given:Number of moles,$n = 5 \ mol$Initial temperature,$T_1 = 335 \ K$Final temperature,$T_2 = 415 \ K$Molar heat capacity at constant volume,$C_{v,m} = 12 \ J \ K^{-1} \ mol^{-1}$Gas constant,$R = 8.3 \ J \ K^{-1} \ mol^{-1}$Step $1$: Calculate the molar heat capacity at constant pressure $(C_{p,m})$.$C_{p,m} = C_{v,m} + R = 12 + 8.3 = 20.3 \ J \ K^{-1} \ mol^{-1}$Step $2$: Calculate the total change in enthalpy $(\Delta H)$.$\Delta H = n 	imes C_{p,m} 	imes (T_2 - T_1)$$\Delta H = 5 	imes 20.3 	imes (415 - 335)$$\Delta H = 5 	imes 20.3 	imes 80$$\Delta H = 8120 \ J$

Column-$1$	Column-$2$
$P$: Process-$I$	$A$: Adiabatic
$Q$: Process-$II$	$B$: Isobaric
$R$: Process-$III$	$C$: Isochoric
$S$: Process-$IV$	$D$: Isothermal

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Column-$1$ Column-$2$
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