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(A) For an isobaric process,the heat supplied is given by $\Delta Q = \mu C_p \Delta T$. According to the first law of thermodynamics,$\Delta Q = \Del

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$2/5$

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(A) For an isobaric process,the heat supplied is given by $\Delta Q = \mu C_p \Delta T$. According to the first law of thermodynamics,$\Delta Q = \Delta U + \Delta W$,where $\Delta U = \mu C_v \Delta T$ is the change in internal energy and $\Delta W$ is the work done. Thus,$\Delta W = \Delta Q - \Delta U = \mu C_p \Delta T - \mu C_v \Delta T = \mu (C_p - C_v) \Delta T$. The fraction of heat converted into work is $f = \frac{\Delta W}{\Delta Q} = \frac{\mu (C_p - C_v) \Delta T}{\mu C_p \Delta T} = 1 - \frac{C_v}{C_p} = 1 - \frac{1}{\gamma}$. For a monoatomic gas,the adiabatic index $\gamma = 5/3$. Therefore,$f = 1 - \frac{1}{5/3} = 1 - \frac{3}{5} = \frac{2}{5}$.

$A$ quantity of heat $Q$ is supplied to a monoatomic ideal gas which expands at constant pressure. The fraction of heat that goes into work done by the gas is

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