Answer :
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 [tex]MnO_2[/tex] and HCl follows:
[tex]MnO_2(s)+4HCl(aq.)\rightarrow Cl_2(g)+MnCl_2(aq.)+2H_2O(l)[/tex]
By Stoichiometry of the reaction:
If 4 moles of HCl produces 1 mole of chlorine gas
So, 1.82 moles of HCl will produce = [tex]\frac{1}{4}\times 1.82=0.455mol[/tex] of chlorine gas
Hence, 0.455 moles of chlorine gas is formed.