Question

Which is the limiting reactant when 3.00 mol of mno2 are reacted with 10.0 mol of hcl in the following equation?mno2 4hcl → mncl2 2h2o cl2

Answer 1

Answer:

Hydrochloric acid - HCl.

Explanation:

Hello,

In this case, by rewriting the undergoing chemical reaction we've got:

$MnO_2+4HCl \rightarrow MnCl_2+2H_2O+Cl_2$

For determining the limiting reagent, one compares the moles of manganese dioxide with those of the hydrochloric acid, for instance, by finding the moles of the MnO₂ that completely react with 10.0 moles of HCl as given on the statement as shown below:

$n_{MnO_2}^{consumed}=10.0molHCl*\frac{1molMnO_2}{4molHCl}=2.5molMnO_2$

In such a way, since 2.5 moles of MnO₂ would be consumed but 3.0 moles are available, there will be 0.5 unreacted moles of it, therefore, the limiting reagent is the hydrochloric acid, HCl as it will be firstly consumed.

Best regards.

Answer 2

The limiting reactant in the reaction would be the compound that would be consumed completely in the reaction. The balanced chemical reaction for this problem is written as:

MnO2 + 4HCl → MnCl2 + 2H2O + Cl2

From the reaction and the amounts present of the reactant, the limiting reactant would be HCl or hydrochloric acid. Ten moles of HCl only need 2.5 moles of MnO2. Hope this helps.