1 mole of an ideal gas expand isothermally and reversibly from a pressure 7 atm to 1 atm at 25°C. What will be the total work done by the system?

Question

1 mole of an ideal gas expand isothermally and reversibly from a pressure 7 atm to 1 atm at 25°C. What will be the total work done by the system? (A) -4822 J (B) 4822 J (C) 3915 J  (D) -3915 J

Tardigrade Admin · Accepted Answer

Work done by the system = -2.303 nRT log (P1/P2) = - 2.303 × 1 × 8.314 × 298 log (7/1) = -2.303 × 1 × 8.314 × 298 × 0.845 = -4822 J

Q. $1$ mole of an ideal gas expand isothermally and reversibly from a pressure $7$ atm to $1$ atm at $2 5^{\circ} C$ . What will be the total work done by the system?

$- 4822 J$

$4822 J$

$3915 J$

$- 3915 J$

Work done by the system
$= - 2.303 n RT l o g \frac{P _{1}}{P _{2}}$
$= - 2.303 \times 1 \times 8.314 \times 298 l o g \frac{7}{1}$
$= - 2.303 \times 1 \times 8.314 \times 298 \times 0.845$
$= - 4822 J$

Q. 1 mole of an ideal gas expand isothermally and reversibly from a pressure 7 atm to 1 atm at 25∘C. What will be the total work done by the system?

−4822J

4822J

3915J

−3915J