Find the isothermal irrevesible work done when 2 moles of hydrogen expand from 15 to 50 litres against a constant pressure of 1 atm at $25^{o} C .$

-848.2 cal

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848.2 kcal

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-84.7 cal

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84.7 kcal

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Solution

The correct option is A -848.2 cal
The formula of work done (W) for an Isothermal Irreversible expansion is
$W = - P (V_{2} - V_{1})$
Where $V_{1}$ is the initial volume of the gas $= 15 L$
$V_{2}$ is the final volume of the gas $= 50 L$

$W = - 1 a t m \times (50 - 15) L = - 35 L a t m$
$W = - 35 \times 101.3 J = - 3545.5 J ∵ (1 L - a t m = 101.3 J)$
$W = - \frac{3545.5}{4.18} ∵ (1 c a l = 4.18 J) = - 848.2 c a l$

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