5 moles of an ideal gas at 27° C expands isothermally and reversibly from a volume of 5 L to 50 L . The work done by the system is

Question

5 moles of an ideal gas at 27° C expands isothermally and reversibly from a volume of 5 L to 50 L . The work done by the system is (A) -14.7 kJ (B) -28.72 kJ (C) 27.72 kJ (D) -56.72 kJ

Tardigrade Admin · Accepted Answer

W=-2.303 nRT log(V2/V1) =-2.303× 5× 8.314× 300× log(50/5) = -28.72 KJ

Q. 5 moles of an ideal gas at $2 7^{\circ} C$ expands isothermally and reversibly from a volume of $5 L$ to $50 L$ . The work done by the system is

$- 14.7 k J$

$- 28.72 k J$

$27.72 k J$

$- 56.72 k J$

$W = - 2.303 n RT l o g \frac{V _{2}}{V _{1}}$
$= - 2.303 \times 5 \times 8.314 \times 300 \times l o g \frac{50}{5}$ = -28.72 KJ

Q. 5 moles of an ideal gas at 27∘C expands isothermally and reversibly from a volume of 5L to 50L . The work done by the system is

−14.7kJ

−28.72kJ

27.72kJ

−56.72kJ