Question

A 0.216 g sample of an aluminium compound X reacts with an excess of water to produce a single hydrocarbon gas. This gas burns completely in O2 to form H2O and CO2 only. The volume of CO2 at room temperature and pressure is 108cm3 . What is the formula of X

Answer 1

Given :

A 0.216 g sample of an aluminium compound X reacts with an excess of water to produce a single hydrocarbon gas.

This gas burns completely in O2 to form H2O and CO2 only.

The volume of CO2 at room temperature and pressure is 108cm³.

To find :

The formula of x = ?

Solution :

$\sf \dfrac {0.108}{n} \ = \ \dfrac {24}{1}$

Therefore,

n = 0.0045 mole.

$\implies \sf 0.216 \ - \ 0.0045$

$\implies \sf 0.2115$

Now,

$\sf Al \ = \ \dfrac {0.2115}{27}$

$\implies \sf 0.0078 \ mole.$

$\sf C \ = \ 0.0045 \times 1000$

$\implies \sf 4.5$

$Al \ = \ 0.0078 \times 1000$

$\implies \sf 7.8$