Final answer:
The question pertains to the mass of chlorine produced from the reaction of hydrochloric acid and manganese(IV) oxide. By writing the balanced chemical equation, converting the given mass of hydrochloric acid to moles, and using stoichiometry, the mass of chlorine gas produced can be calculated.
Step-by-step explanation:
The student asks about the production of chlorine gas from the reaction of hydrochloric acid and manganese(IV) oxide. To find the mass of chlorine that can be produced, we must first write the balanced chemical equation for the reaction:
MnO₂(s) + 4HCl(aq) → MnCl₂(aq) + 2H₂O(l) + Cl₂(g)
From the balanced equation, we can see that 4 moles of HCl produce 1 mole of Cl₂. Now we need to convert the given mass of HCl to moles:
Mass of HCl = 4.76 × 10⁻² g
The molar mass of HCl is approximately 36.46 g/mol.
Moles of HCl = Mass of HCl / Molar mass of HCl = 4.76 × 10⁻² g / 36.46 g/mol
Once we have the moles of HCl, we can find the moles of Cl₂ produced by using the stoichiometric ratio from the balanced equation, and then convert the moles of Cl₂ to grams using the molar mass of Cl₂:
Molar mass of Cl₂ = 2 × 35.45 g/mol
Finally, we calculate the mass of Cl₂ produced from the stoichiometry of the reaction.