In a constant pressure process for 5 text{ mo | vedclass

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(C) For an ideal monoatomic gas,$C_{v,m} = \frac{3}{2} R$ and $C_{p,m} = \frac{5}{2} R$.$\Delta H = n C_{p,m} \Delta T = 5 	imes \frac{5}{2} R 	imes

Vedclass · Accepted Answer

$q = 3500 \ R$

Vedclass · Answer

(C) For an ideal monoatomic gas,$C_{v,m} = \frac{3}{2} R$ and $C_{p,m} = \frac{5}{2} R$.$\Delta H = n C_{p,m} \Delta T = 5 	imes \frac{5}{2} R 	imes (500 - 300) = 5 	imes 2.5 R 	imes 200 = 2500 \ R$.$\Delta U = n C_{v,m} \Delta T = 5 	imes \frac{3}{2} R 	imes (500 - 300) = 5 	imes 1.5 R 	imes 200 = 1500 \ R$.At constant pressure,$q_p = \Delta H = 2500 \ R$.Using the first law of thermodynamics,$\Delta U = q_p + w$,so $w = \Delta U - q_p = 1500 \ R - 2500 \ R = -1000 \ R$.Comparing these results with the given options,option $C$ $(q = 3500 \ R)$ is incorrect.

In a constant pressure process for $5 \text{ mole}$ of an ideal monoatomic gas,the temperature of the gas increased from $300 \ K$ to $500 \ K$. Which of the following is incorrect regarding the process?

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