Chlorine gas can be made from the reaction of manganese dioxide with hydrochloric acid. MnO₂(s) + 4HCl(aq) $\rarr$ MnCl₂(aq) + 2H₂O(l) + Cl₂(g)
According to the above reaction, deterrmine the limiting reactant when 5.6 moles of MnO₂ are reacted with 7.5 moles of HCl?

Question

Chlorine gas can be made from the reaction of manganese dioxide with hydrochloric acid. MnO₂(s) + 4HCl(aq)

\rarr

MnCl₂(aq) + 2H₂O(l) + Cl₂(g)
According to the above reaction, deterrmine the limiting reactant when 5.6 moles of MnO₂ are reacted with 7.5 moles of HCl?

Quizplus · Accepted Answer

To determine the limiting reactant, we need to calculate the moles of product formed by each reactant and identify the one that produces the smallest amount of product.

5.6 moles of MnO2 react with 4 x 5.6 = 22.4 moles of HCl (according to the stoichiometry of the equation).
However, we only have 7.5 moles of HCl available, which means it is the limiting reactant.

Using 7.5 moles of HCl, we can calculate the moles of product formed:
7.5 moles of HCl x 1 mole of MnCl2/4 moles of HCl = 1.875 moles of MnCl2

This means that MnO2 is in excess, while HCl is completely consumed. Therefore, the limiting reactant is HCl.

Chlorine Gas Can Be Made from the Reaction of Manganese →\rarr→

Chlorine Gas Can Be Made from the Reaction of Manganese $\rarr$