Question

(05 06 MC) The theoretical yields of Cl2 from certain starting amounts of MnO2 and HCl were calculated as 65.36 g and 68.08 g, respectively.

If the percentage yield of Cl2 is 70%, what is its actual yield?

42.25g
45.65g
46.33g
47.66g​

Answer 1

Actual yield : 45.752 g ⇒no option

Further explanation

Given

The theoretical yields of Cl₂ : 65.35 g and 68.08 g

Required

The actual yield

Solution

Reaction

4 HCl (aq) + MnO₂ (s) → MnCl₂ (aq) + Cl₂ (g) + 2H₂O (l)

Because there are two theoretical yields, then we can choose the smallest one because the value is usually determined from the limiting reactant (in this reaction the limiting reactant is MnO₂)

So 65.36 g is The theoretical yields of Cl₂

Then the actual yield :

`\tt \%yield=(actual)/(theoretical)* 100\%\\\\actual=\%yield* theoretical\\\\actual=70\%* 65.36=45.752`