Question

When 1.82 moles of HCL reacts with excess MnO2, how many moles of Cl2 form

Answer 1

The balanced reaction is:

MnO2(s) + 4HCl(aq) → Cl2(g) + MnCl2(aq) + 2H2O(l)

We are given the amount of hydrochloric acid to be used for the reaction. This will be the starting point for the calculations.

1.82 mol HCl ( 1 mol Cl2 / 4 mol HCl) = 0.46 mol Cl2

Therefore, 0.46 mol of chlorine gas is produced for the reaction of hydrochloric acid and manganese oxide.

Answer 2

Answer: 0.455 moles of chlorine gas is formed.

Explanation:

We are given:

Moles of HCl = 1.82 moles

The chemical equation for the reaction of $MnO_2$ and HCl follows:

$MnO_2(s)+4HCl(aq.)\rightarrow Cl_2(g)+MnCl_2(aq.)+2H_2O(l)$

By Stoichiometry of the reaction:

If 4 moles of HCl produces 1 mole of chlorine gas

So, 1.82 moles of HCl will produce = $\frac{1}{4}\times 1.82=0.455mol$ of chlorine gas

Hence, 0.455 moles of chlorine gas is formed.