Chlorine forms from the reaction of hydrochloric acid with manganese(iv) oxide. calculate the theoretical yield and the percent of chlorine if 86.0g of mno2 and 50.0g of hcl react. the actual yield of cl2 is 20.0g.

Explanation:

We are given the masses of two reactants and asked to determine the mass of the product.

This looks like a limiting reactant problem.

1. Assemble the information

We will need a balanced equation with masses and molar masses, so let’s gather all the information in one place.  

MM:          86.94    36.46                 70.91

                MnO₂ + 4HCl ⟶ MnCl₂ + Cl₂ + 2H₂O

Mass/g:     86.0      50.0                  20.00

2. Calculate the moles of each reactant

3. Calculate the moles of Cl₂ formed from each reactant

From MnO₂:

From HCl:

4. Identify the limiting reactant

The limiting reactant is HCl, because it forms fewer moles of Cl₂.

5. Calculate the theoretical yield of Cl₂

6. Calculate the percentage yield of Cl₂

the atomic mass is the bottom number on the element.

-steel jelly

frequency, z, and the collision density, z, in carbon dioxide (co2), r 180 pm at 30 °c and 120 kpa