Title: Quick % Yield Introduction Example Overview
Course: Stoichiometry

The Make-Up of a % Yield Problem

An example problem:

2 H_2 + O_2 -----> 2 H_2O
In the laboratory, 30.0 g of H_2 was reacted with excess O_2 and 200. g of H_2O was produced. What is the % yield of the H_2O?

Actual Yield:

The actual yield is usually given in the problem statement (If it is not, then the % yield must be given in the problem statement). Notice that the question asks about the % yield of H_2O. That means that the number that relates to the H_2O is the actual yield.

200. g of H_2O is the actual yield in this case.

Theoretical Yield:

Be careful, the 30.0 g of H_2 IS NOT the theoretical yield! You have to use it to get the theoretical yield. You can do a mass - mass problem between H_2 and H_2O to determine the theoretical yield of H_2O (268 g of H_2O).

Percent Yield:

% Yield = 100 x (200/268) = 74.7% Yield

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