The reaction between aluminium and chlorine gas is:

$2\,\mathrm{Al} + 3\,\mathrm{Cl_2} \rightarrow 2\,\mathrm{AlCl_3}$

A sample of aluminium weighing 5.0 g is only 90 % pure, and 4.0 g of chlorine gas is used.

(i) Determine the limiting reagent.

(ii) Calculate the theoretical mass of aluminium chloride ($\mathrm{AlCl_3}$) that could be produced.

(iii) If the actual mass of $\mathrm{AlCl_3}$ obtained after the reaction is 4.0 g, calculate the percent yield.

Question

The reaction between aluminium and chlorine gas is:

$2\,\mathrm{Al} + 3\,\mathrm{Cl_2} \rightarrow 2\,\mathrm{AlCl_3}$

A sample of aluminium weighing 5.0 g is only 90 % pure, and 4.0 g of chlorine gas is used.

(i) Determine the limiting reagent.

(ii) Calculate the theoretical mass of aluminium chloride ($\mathrm{AlCl_3}$) that could be produced.

(iii) If the actual mass of $\mathrm{AlCl_3}$ obtained after the reaction is 4.0 g, calculate the percent yield.

Accepted Answer

Limiting reagent: Cl₂; theoretical yield ≈ 5.0 g AlCl₃; percent yield ≈ 80 %

Igcse Model Questions Vol1 2023 Chemistry Question 5