Question

one mole of ocygen is allowed to expand isothermally and reversibly from 5 m^3 to 10m^3 at 300 k calculate the work done in expansion of the gas

Answer 1

Answer : The work done in expansion of the gas is, -1728.84 J

Solution :

Formula used for isothermal reversible ideal gas is,

$w=-nRT\ln (\frac{V_2}{V_1})$

where,

w = work done

n = number of moles of gas = 1 mole

R = gas constant = 8.314 J/moleK

T = temperature of gas = 300 K

$V_1$ = initial volume of gas = $5m^3$

$V_2$ = final volume of gas = $10m^3$

Now put all the given values in the above formula, we get the work done.

$w=-[(1mole)\times (8.314J/moleK)\times (300K)]\ln (\frac{10}{5})$

$w=-1728.84J$

Therefore, the work done in expansion of the gas is, -1728.84 J