When 2 moles of an ideal gas are expanded iso | vedclass

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(A) Given: $n = 2 \ mol$,$V_{1} = 12.5 \ L = 12.5 	imes 10^{-3} \ m^{3}$,$V_{2} = 15.0 \ L = 15.0 	imes 10^{-3} \ m^{3}$,$P_{ext} = 760 \ mm \ Hg =

Vedclass · Accepted Answer

$-253.25$

Vedclass · Answer

(A) Given: $n = 2 \ mol$,$V_{1} = 12.5 \ L = 12.5 	imes 10^{-3} \ m^{3}$,$V_{2} = 15.0 \ L = 15.0 	imes 10^{-3} \ m^{3}$,$P_{ext} = 760 \ mm \ Hg = 1.013 	imes 10^{5} \ N \ m^{-2}$.Work done in an irreversible expansion is given by the formula: $W = -P_{ext} \Delta V$.$W = -P_{ext}(V_{2} - V_{1}) = -1.013 	imes 10^{5} 	imes (15.0 - 12.5) 	imes 10^{-3} \ J$.$W = -1.013 	imes 10^{5} 	imes 2.5 	imes 10^{-3} \ J$.$W = -1.013 	imes 250 \ J$.$W = -253.25 \ J$.

When $2$ moles of an ideal gas are expanded isothermally from a volume of $12.5 \ L$ to $15.0 \ L$ against a constant external pressure of $760 \ mm \ Hg$,calculate the amount of work done in joules. (in $J$)

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