The heat energy that must be supplied to 14 | vedclass

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Question

(B) The heat energy $Q$ supplied at constant pressure is given by the formula $Q = n C_p \Delta T$.First,calculate the number of moles $n$ of nitrogen

Vedclass · Accepted Answer

$84$

Vedclass · Answer

(B) The heat energy $Q$ supplied at constant pressure is given by the formula $Q = n C_p \Delta T$.First,calculate the number of moles $n$ of nitrogen $(N_2)$:$n = \frac{	ext{mass}}{	ext{molecular weight}} = \frac{14 \ g}{28 \ g/mol} = 0.5 \ mol$.Given the change in temperature $\Delta T = 48^{\circ} C$ and the molar heat capacity at constant pressure $C_p = \frac{7}{2} R$.Substituting these values into the formula:$Q = 0.5 	imes \left(\frac{7}{2} Right) 	imes 48$.$Q = 0.5 	imes 3.5 R 	imes 48$.$Q = 1.75 R 	imes 48 = 84 R$.Therefore,the heat energy supplied is $84 R$.

The heat energy that must be supplied to $14 \ g$ of nitrogen at room temperature to raise its temperature by $48^{\circ} C$ at constant pressure is (Molecular weight of nitrogen $= 28, R =$ gas constant,$C_p = \frac{7}{2} R$ for diatomic gas). (in $R$)

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