The density of the vapour of a substance at 1 atm pressure and 500 K is 0.36 kg `m^(-3)`. The vapour effuses through a small hole at a rate of 1.33 times faster than oxygen under the same condition.
Determine, (a) molecular weight (b) molar volume (c) compression factor (Z) of the vapour and (d) which forces among the gas molecules are dominating, the attractive or the repulsive?

Explanation

To solve the given problem step by step, we will address each part of the question sequentially.

### Step 1: Determine the Molecular Weight (M)
To find the molecular weight of the vapor, we can use Graham's law of effusion, which states that the rate of effusion of a gas is inversely proportional to the square root of its molar mass.

**Formula:**
\[
\frac{R_1}{R_2} = \sqrt{\frac{M_2}{M_1}}
...