The van der Waal's equation of state for 1 mole real gas is `(P + (a)/(V^(2))) (v - b) = RT`....(i)
The Virial equation for 1 mole real gas is `PV = RT [1 + (x)/(V) + (y)/(V^(2)) + (z)/(V^(3))+....." To higher power of " V]` ....(ii)
when x, y and z are constants which are known as 2nd, 3rd adn 4th co-efficients respectively. The temperature at which real gas obeys ideal gas equation i.e., `(PV = nRT)` is known as Boyle's temperature.
Answer the following questions on the basis of the above write up :
Which of the following is the incorrect statement about the Boyle's temperature ?

Options

A. Temperature at which first virial co-efficient become zero
B. Temperature of which first virial coefficient is RT
C. Temperature at which third virial co-efficient vanishes
D. Both A and C

Answer

A

Explanation

Second virial co-efficient becomes zero and not the third