Answer:
c 43.38 g
Explanation:
The reaction between MnO2 and HCl can be represented by the following balanced equation:
MnO2 + HCl ---> Cl2 + MnCl2 + H2O
From the balanced equation, the theoretically required molar ratio of MnO2 to HCl is 1:1, therefore the yields would have been expected to be equal.
For the fact that HCl gives a higher yield (65.02g) than MnO2 (60.25g) according to the problem statement, HCl should be in excess, while the limiting reagent should be MnO2 .
Thus, the theoretical yield of Cl2 will be 60.25 g.
By definition, the percentage yield is given by
% Yield = (Actual Yield) / (Theoretical Yield),
This can be simplified to
Actual Yield = % Yield * Theoretical Yield
Plugging in the given values we have
Actual Yield = 72% * 60.25 = 43.38 g
