To increase the temperature of 2 moles of an | vedclass

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(B) The heat supplied at constant pressure is given by $(\Delta Q)_P = \mu C_P \Delta T$.Given $\mu = 2 \, mol$,$\Delta T = (35 - 30) = 5 \, K$,and $(

Vedclass · Accepted Answer

$50$

Vedclass · Answer

(B) The heat supplied at constant pressure is given by $(\Delta Q)_P = \mu C_P \Delta T$.Given $\mu = 2 \, mol$,$\Delta T = (35 - 30) = 5 \, K$,and $(\Delta Q)_P = 70 \, cal$.Substituting these values: $70 = 2 	imes C_P 	imes 5 \Rightarrow C_P = 7 \, cal/mol \cdot K$.Using Mayer's relation,$C_P - C_V = R$,we find $C_V = C_P - R = 7 - 2 = 5 \, cal/mol \cdot K$.The heat required at constant volume is $(\Delta Q)_V = \mu C_V \Delta T$.Substituting the values: $(\Delta Q)_V = 2 	imes 5 	imes 5 = 50 \, cal$.

To increase the temperature of $2$ moles of an ideal gas by $30^{\circ}C$ to $35^{\circ}C$ at constant pressure,$70 \, cal$ of heat is required. How much heat energy in $cal$ is required to increase the temperature by the same amount at constant volume? $(R = 2 \, cal/mol \cdot K)$

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