Percentage Yield
yield can be in g or mol
% Yield = Actual Yield x 100 Jens Martensson
Theoretical Yield
Theoretical yield - The amount of product predicted by the balanced
equation when all the limiting reactant has reacted .
Actual yield - The amount of product actually obtained from a reaction.
Percentage Yield
EXAMPLE: H2 + F2 2HF
3 mol 2 mol
4 mol
(theoretical yield) Jens Martensson
3.5 mol
(actual yield) actually produced!
Given that F2 is limiting reactant,
4 mol of HF is expected to be produced => Theorectical yield
but only 3.5 mol of HF is actually produced => Actual yield
% Yield = 3.5 mol x 100 = 87.5 %
4 mol
YTohuank Prepared by Miss Eva
Kolej Matrikulasi Johor
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1.1 ATOMS AND MOLECULES
1.2 MOLE CONCEPT
1.3 STOICHIOMETRY
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