Two litres of an ideal gas at a pressure of 1 | vedclass

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(A) For an expansion into a vacuum,the external pressure $p_{ex} = 0 \ atm$.The work done in an expansion is given by $w = -p_{ex} \Delta V$.Since $p_

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$q = 0, w = 0$

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(A) For an expansion into a vacuum,the external pressure $p_{ex} = 0 \ atm$.The work done in an expansion is given by $w = -p_{ex} \Delta V$.Since $p_{ex} = 0$,the work done $w = 0 \ L \ atm$.According to the first law of thermodynamics,$\Delta U = q + w$.For an isothermal expansion of an ideal gas,the change in internal energy $\Delta U = 0$.Therefore,$0 = q + 0$,which implies $q = 0$.Thus,no work is done and no heat is absorbed.

Two litres of an ideal gas at a pressure of $10 \ atm$ expands isothermally at $25^{\circ}C$ into a vacuum until its total volume is $10 \ litres$. How much heat is absorbed and how much work is done in the expansion?

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