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What is Boyle's temperature?...

What is Boyle's temperature?

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The temperature at which a real gas behaves like an ideal gas over an appreciable pressure range is called Boyle temperature or Boyle point.
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At Boyle temperature

Boyle's temperature (T_(B)) : It is the temperature at which a real gas exhibits ideal behavior in low pressure range. Different gases have different value of T_(B) , which is related to the van der Wall's constant a and ab as follows: T_(B) = (a)/(Rb) The compressiblity factor for a real gas is given as Z = 1 + 0.35 P - (168)/(T)P . Where P is in bar and T is in Kelvin. What is the Boyle's temperature of the gas?

The ratio of Boyle's temperature and critical temperature for a gas is:

The Critical temperature , Boyle's temperature and inversion temperature respectively are given as

The ratio of the inversion temperature of a gas to its Boyle temperature is

Inversion temperature (T_(i)=(2a)/(Rb)) is defined as the temperature above which if gas is expanded adiabatically it gets warm up but if temperature of gas is lower than T_(i) then it will cool down. What will happen to gas if it is adiabatically expanded at 50^(@)C if its Boyle's temperature is 20^(@)C

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) ) Plot at Boyle's temperature for the gas will be

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) ) Which of the following is correct :

The van der Waals' constantes for a gas are a=3.6 atmL^(2)mol^(-2),b=0.6Lmol^(-1) .If R=0.08LatmK^(-1)mol^(-1) and the Boyle's temperature (K) is T_(B) of this gas, then what is the value of (T_(B))/(15) ?

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) ) For 500 K plot value of Z changes from 2 to 2.2 if pressure is varied from 1000 atm to 1200 atm (high pressure ) then the value of b/(RT) will be

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