Question

The reduced temperature for benzene is 0.7277 and its reduced volume is 0.40. Calculate the reduced pressure of benzene.

• A. $40.358$
• B. $30.358$
• C. $20.358$
• D. $10.358$

Answer 1

The correct option is D $10.358$

Given: $T_r=0.7277$
$V_r=0.40$
$P_r=?$
From Van der Waals equation for reduced state,
$[P_r+\frac{3}{V_r^2}][3V_r-1]=8T_r$
$\Rightarrow [P_r+\frac{3}{(0.40{)}^2}][3\times 0.4-1]=8\times 0.7277$
$\Rightarrow P_r+\frac{3}{0.16}=29.108$
$\Rightarrow P_r+18.75=29.108$
$\Rightarrow P_r=10.358$