Sketch shows the plot of Z v/s P for a hypothetical gas for one mole at three distint temperature. Boyle's temperature is the temperature at which gas shows ideal behaviour over a pressure range in the low pressure region.Boyle's temperature (T_b)=a/(Rb).If a plot is obtained at temperature well below Boyle's temperature then the curve will show negative deviation, in low pressure region and positive deviation in the high pressure region. Near critical temperature the curve is more likely as CO_2 and the temperature well above critical temperature curve is more like H_2 at 0^@C as shown above.At high pressure suppose all the constant temperature curve varies linearly with pressure according to the following equation : Z=1+(Pb)/(RT) (R=2 cal "mol"^(-1) K^(-1)) As shown in the figure at 200 K and 500 atm value of compressibility factor is 2 (approx).Then volume of the gas at the point will be

Sketch shows the plot of Z v/s P for a hypothetical gas for one mole a

1.	Sketch shows the plot of Z v/s P for a hypothetical gas for one mole at three distint temperature. Boyle's temperature is the temperature at which gas shows ideal behaviour over a pressure range in the low pressure region.Boyle's temperature (T_b)=a/(Rb).If a plot is obtained at temperature well below Boyle's temperature then the curve will show negative deviation, in low pressure region and positive deviation in the high pressure region. Near critical temperature the curve is more likely as CO_2 and the temperature well above critical temperature curve is more like H_2 at 0^@C as shown above.At high pressure suppose all the constant temperature curve varies linearly with pressure according to the following equation : Z=1+(Pb)/(RT) (R=2 cal "mol"^(-1) K^(-1)) As shown in the figure at 200 K and 500 atm value of compressibility factor is 2 (approx).Then volume of the gas at the point will be
Answer» <P>0.01 L 0.09L 0.065 L 0.657 L Solution :USE `z=(PV_(m))/(RT)IMPLIES V_m=(z.RT)/P`