The sketch shows the plot of Z vs P for 1 mole of a hypothetical gas at three distincttemperatures:Boyle's temperature is the temperature at which a gas shows ideal behaviour over apressure range in the low pressure region. Boyle's temperature (Tb)=aRb. If a plot isobtained at temperatures well below Boyle's temperature, then the curve will show a negative deviation in the low pressure region and a positive deviation in the high pressureregion. In the first figure, in the plot at 500 K,Z changes from 2 to 2.2 as the pressure varies from 1000 atm to 1200 atm (high pressure). The value of bRT will be:

The sketch shows the plot of Z vs P for 1 mole of a hypothetical gas a

1.	The sketch shows the plot of Z vs P for 1 mole of a hypothetical gas at three distincttemperatures:Boyle's temperature is the temperature at which a gas shows ideal behaviour over apressure range in the low pressure region. Boyle's temperature (Tb)=aRb. If a plot isobtained at temperatures well below Boyle's temperature, then the curve will show a negative deviation in the low pressure region and a positive deviation in the high pressureregion. In the first figure, in the plot at 500 K,Z changes from 2 to 2.2 as the pressure varies from 1000 atm to 1200 atm (high pressure). The value of bRT will be:
Answer» The sketch shows the plot of Z vs P for 1 mole of a hypothetical gas at three distinct temperatures: Boyle's temperature is the temperature at which a gas shows ideal behaviour over a pressure range in the low pressure region. Boyle's temperature $(T_{b}) = \frac{a}{R b}$ . If a plot is obtained at temperatures well below Boyle's temperature, then the curve will show a negative deviation in the low pressure region and a positive deviation in the high pressure region. In the first figure, in the plot at $500 K, Z$ changes from 2 to 2.2 as the pressure varies from 1000 atm to $1200 atm$ (high pressure). The value of $\frac{b}{R T}$ will be: