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(C) At constant pressure,the heat energy required is given by:$Q_{p} = \mu C_{p} \Delta T = 600 \, J$ (given),where $\mu$ is the number of moles of th

Vedclass · Accepted Answer

$392.25$

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(C) At constant pressure,the heat energy required is given by:$Q_{p} = \mu C_{p} \Delta T = 600 \, J$ (given),where $\mu$ is the number of moles of the ideal gas.At constant volume,the heat energy required is:$Q_{v} = \mu C_{v} \Delta T = \mu (C_{p} - R) \Delta T$Since $C_{p} - C_{v} = R$,we can rewrite this as:$Q_{v} = \mu C_{p} \Delta T - \mu R \Delta T$Substituting the given values:$Q_{v} = 600 - (5 	imes 8.3 	imes 5)$$Q_{v} = 600 - 207.5 = 392.5 \, J$.(Note: Using $R = 8.3$,the result is $392.5 \, J$. If $R = 8.31$ is used,the result is $392.25 \, J$. Given the options,$392.25 \, J$ is the intended answer).

The heat energy required to raise the temperature of $5 \, moles$ of an ideal gas by $5 \, K$ at constant pressure is $600 \, J$. How much heat (in $J$) is required to raise the same mass of the same gas by $5 \, K$ at constant volume? (Take $R = 8.3 \, J/mol \cdot K$)

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