Two moles of helium gas expanded isothermally and irreversibly at 27o textC from volume 1 dm3 to 1 m3 at constant pressure of text100 k Pa. Calculate the work done.

Question

Two moles of helium gas expanded isothermally and irreversibly at 27o textC from volume 1 dm3 to 1 m3 at constant pressure of text100 k Pa. Calculate the work done. (A)  text99900 J (B) - text99900 J  (C)  text34464 text.65 J (D) - text34464 text.65 J

Tardigrade Admin · Accepted Answer

textW=- textP∆V Given, textP = 1 0 0 text k textPa = 1 05 textPa textV1=1 text d textm3=10- 3 textm3, textV2=1 text m3 mathrmW=-105 ×(1-10-3) mathrmJ ∴ text W = - 99900 textJ

Q. Two moles of helium gas expanded isothermally and irreversibly at $2 7^{o} C$ from volume $1 d m^{3}$ to $1 m^{3}$ at constant pressure of $100 k Pa .$ Calculate the work done.

$99900 J$

$- 99900 J$

$34464 .65 J$

$- 34464 .65 J$

$W = - P∆ V$

Given, $P = 100 k Pa = 1 0^{5} Pa$

$V_{1} = 1 d m^{3} = 1 0^{- 3} m^{3}, V_{2} = 1 m^{3}$

$W = - 1 0^{5} \times (1 - 1 0^{- 3}) J$

$∴ W = - 99900 J$

Q. Two moles of helium gas expanded isothermally and irreversibly at 27oC from volume 1dm3 to 1m3 at constant pressure of 100 k Pa. Calculate the work done.

99900 J

−99900 J

34464.65 J

−34464.65 J