Verified Answer :

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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: 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.

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