Two moles of an ideal gas is expanded isother | vedclass

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(A) The work done in an irreversible isothermal expansion against constant external pressure is given by the formula: $W = -P_{ext} \Delta V$. Given:

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$-418$

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(A) The work done in an irreversible isothermal expansion against constant external pressure is given by the formula: $W = -P_{ext} \Delta V$. Given: $V_1 = 300 \ cm^3 = 0.3 \ dm^3$ (since $1 \ dm^3 = 1000 \ cm^3$). $V_2 = 2.5 \ dm^3$. $P_{ext} = 1.9 \ bar$. $\Delta V = V_2 - V_1 = 2.5 \ dm^3 - 0.3 \ dm^3 = 2.2 \ dm^3$. $W = -1.9 \ bar 	imes 2.2 \ dm^3 = -4.18 \ bar \cdot dm^3$. Since $1 \ bar \cdot dm^3 = 100 \ J$,$W = -4.18 	imes 100 \ J = -418 \ J$.

Two moles of an ideal gas is expanded isothermally from a volume of $300 \ cm^3$ to $2.5 \ dm^3$ at $298 \ K$ against a constant pressure of $1.9 \ bar$. Calculate the work done in joules. (in $J$)

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