`10mol` of an ideal gas confined to a volume of `10L` is released into atmosphere at `300K` where the pressure is 1bar. The work done by the gas is `(R = 0.083 L "bar" K^(-1)mol^(-1))`

10 moles of an ideal gas confined to a volume of 10 L is released into atmosphere at 300 K where the pressure is 1 bar. The work done by the gas is: ltBrgt (R=0.083L" bar "K^(-1)mol^(-1))

20 mol of chlorine gas occupies a volume of 800 mL at 300 K and 5xx10^(6) Pa pressure. Calculate the compressibility factor of the gas. (R=0.083 L "bar" K^(-1)mol^(-1)) . Comment, whether the gas is more compressible or less compressible under these conditions.

An ideal gas is allowed to expand from 1 L to 10 L against a constant external pressure of 1 bar. Calculate the work done inkJ.

20 mol of chlorine gas occupies a volume of 800 ml at 300 K and 5 xx 10^(6) Pa pressure. Calculate the compressibility factor of the gas (R = 0.083 L bar K^(-1) mol^(-1) ). Comment whether the gas is more compressible or less compressible under the conditions

2 mol of chlorine gas occupies a volume of 800 mL at 300 K and 5xx10^(6) Pa pressure. Calculate the compressibility factor of the gas. (R=0.083 L "bar" K^(-1)mol^(-1)) . Comment, whether the gas is more compressible or less compressible under these conditions.

20 mol of chlorine gas occupies a volume of 800 ml at 300 K and 5 xx 10^(6) Pa pressure. Calculate the compressibility factor of the gas (R = 0.083 L bar K^(-1) mol^(-1) ). Comment whether the gas is more compressible or less compressible under the conditions

Three grams of non - volatile solute whenn dissolved in a litre of water shows an osmotic pressure of 2 bar at 300K. Calculate the molar mass of the solute . (R = 0.083 L bar K^(-1) mol^(-1) ) .