# 0.314 mol of a diatomic molecule has a mass of 22.26g. How would you identify the molecule?

Aug 23, 2017

We take the quotient $\text{mass"/"molar quantity}$............, and we indentify the molecule as $C {l}_{2}$........

#### Explanation:

And thus $\text{mass"/"molar quantity} = \frac{22.26 \cdot g}{0.314 \cdot m o {l}^{-} 1}$

$\equiv 70.9 \cdot g \cdot m o {l}^{-} 1$ WITH RESPECT TO ${X}_{2}$, and thus the molar mass, with respect to $X$ was $35.45 \cdot g \cdot m o {l}^{-} 1$, and clearly $X = C l$, i.e. ${X}_{2} \equiv C {l}_{2}$.

As a tip, which I would expect A2 students, and certainly 1st year undergraduates, to know, $\text{ALL of the elemental gases}$ (save the Noble Gases), $\text{dihydrogen, dinitrogen, dioxygen, dihalogen,}$ are BINUCLEAR, i.e. ${H}_{2}$, ${N}_{2}$, ${X}_{2}$ etc.

And of course $B {r}_{2}$ is a room temperature liquid, and ${I}_{2}$ is a room temperature solid.