Question

The following equations of state are occasionally used for approximate calculation on gases:

Gas (X): PV =RT{1+(b/Vm)}

Gas (Y): P(Vm - b) = RT

Assuming that gas (X) and (Y) actually obeyed above equation of state respectively then choose
the correct statement:
(A) Gas (X) is more liquefiable than Gas (Y)
(B) Gas (X) and (Y) both are liquefiable
(C) Neither Gas (X) nor Gas (Y) is liquefiable
(D) Gas (Y) is more liquefiable than Gas (X)​

Answer 1

Answer:

answer is 55 DD root sfdjdj

Answer 2

Neither Gas(X) nor Gas(Y) is liquefiable

Explanation:

Gas (X): PV =RT{1+($\frac{b}{V_{m} }$)}

Gas (Y): P($V_{m}$ - b) = RT

Here, in the given equation there is no information about a ( indirect measure of forces ).

• a and b are vanderwaal's constant and are very useful for pressure and volume correction.

So b will give the idea of excluded volume per molecule but a gives the idea of forces present in the gas. If there is no information about a then we can not predict about liquiflmability of gases, hence option c is correct.