Percentage yield

An is the mass of a product actually obtained from the reaction. It is usually less than the . The reasons for this include:

incomplete reactions, in which some of the reactants do not react to form the product
practical losses during the experiment, such as during pouring or
side reactions (unwanted reactions that compete with the desired reaction)

Calculating percentage yield

The is calculated using this equation:

\(percentage\ yield\ =\ \frac{actual\ yield}{theoretical\ yield}\ \times\ 100\)

Worked example

Copper oxide reacts with sulfuric acid to make copper sulfate and water. In an experiment, 1.6 g of dry copper sulfate crystals are made. If the theoretical yield is 2.0 g, calculate the percentage yield of copper sulfate.

actual yield = 1.6 g

\(percentage\ yield\ =\ \frac{1.6}{2.0}\ \times\ 100\)

percentage yield = 80%

Question

In an experiment, the theoretical yield is 3.2 g but the actual yield is only 2.4 g. Calculate the percentage yield.

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Monitoring chemical reactions - OCR GatewayPercentage yield