A piston filled with 0.04 mol of an ideal gas expands reversibly from 50.0 mL to 375 mL at a constant temperature of 37.0 °C. As it does so, it absorbs 208 J of heat. The values of q and w for the process will beR=83.14JK−1mol−1,ln⁡7.5=2.01

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A piston filled with $0.04 mol$ of an ideal gas expands reversibly from $50.0 mL to 375 mL$ at a constant temperature of $37.0 ° C$ . As it does so, it absorbs $208 J$ of heat. The values of $q$ and $w$ for the process will be

$(R = 83.14 {JK}^{- 1} {mol}^{- 1}, \ln 7.5 = 2.01)$

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$q = + 208 J, w = 208 J$

$q = + 208 J, w = + 208 J$

$q = - 208 J, w = - 208 J$

$q = - 208 J, w = + 208 J$

answer is A.

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Detailed Solution

For an isothermal expansion of an ideal gas, $Δ U = 0$ . From the first law of thermodynamics, $q = - w$ Since heat is absorbed, $q = 208 J$ and $w = - 208 J$ .