Which is the limiting reactant when 3.00 moles of MnO₂ are reacted with 10.0 moles of HClin the following equation? MnO₂ + 4HCl $\rarr$MnCl₂ + 2H₂O + Cl₂

Question

Quizplus · Accepted Answer

To determine the limiting reactant, we need to compare the moles of each reactant to the balanced equation. From the equation, we can see that 1 mole of MnO₂ reacts with 4 moles of HCl. Therefore, if we have 3.00 moles of MnO₂ and 10.0 moles of HCl, we can see that we have excess HCl. Calculating the theoretical number of moles of MnO₂ needed: 3.00 mol MnO₂ x (4 mol HCl/1 mol MnO₂) = 12.0 mol HCl needed Since we only have 10.0 moles of HCl, it will limit the reaction and be completely consumed, leaving an excess of MnO₂. Therefore, the limiting reactant is HCl (choice B).

Which Is the Limiting Reactant When 3 →\rarr→ MnCl2 + 2H2O + Cl2 A)MnO2 B)HCl C)MnCl2 D)H2O

Which Is the Limiting Reactant When 3 $\rarr$ MnCl₂ + 2H₂O + Cl₂
A)MnO₂
B)HCl
C)MnCl₂
D)H₂O