Calculate the work done when 2 moles of hydrogen expand isothermally and reversibly at 27°C from 15 to 50 litres.

Question

Calculate the work done when 2 moles of hydrogen expand isothermally and reversibly at 27°C from 15 to 50 litres. (A) 14.45 kcal (B) 1445 J (C) 1445 cal (D) 14.45 kJ

Tardigrade Admin · Accepted Answer

W=-2.303 nRT log (V2/V1) =-2.303×2×2×300 log (50/15) =-2763.6(log 10-log 3) =-2763.6(1-0.4771) =-2763.6×0.5229=-1445 cal

Q. Calculate the work done when $2$ moles of hydrogen expand isothermally and reversibly at $2 7^{\circ} C$ from $15$ to $50$ litres.

$14.45 k c a l$

$1445 J$

$1445 c a l$

$14.45 k J$

$W = - 2.303 n RT l o g \frac{V _{2}}{V _{1}}$
$= - 2.303 \times 2 \times 2 \times 300 l o g \frac{50}{15}$
$= - 2763.6 (l o g 10 - l o g 3)$
$= - 2763.6 (1 - 0.4771)$
$= - 2763.6 \times 0.5229 = - 1445 c a l$

Q. Calculate the work done when 2 moles of hydrogen expand isothermally and reversibly at 27∘C from 15 to 50 litres.

14.45kcal

1445J

1445cal

14.45kJ