percentage yield

• Percentage yield is the ratio between actual yield and theoretical yield, expressed as a percentage.
• In chemistry, the amount of product obtained from a chemical reaction is known as the yield, which can be measured in grams or moles.
• The term "actual yield" is used to describe the amount obtained when a chemical reaction is carried out.
• The term "theoretical yield" is used to describe the yield expected based on calculations.
• The percentage yield can range from zero percent if no product is obtained to 100 percent if all products predicted are obtained.
• In a reaction where 2 grams of hydrogen are reacted with 16 grams of oxygen, the theoretical yield is 18 grams but the actual yield is only 15 grams, resulting in a percentage yield of 83.3 percent.
• The percentage yield is calculated by taking the actual yield and dividing it by the theoretical yield, then multiplying it by 100.
• If 2 grams of hydrogen are reacted with 16 grams of oxygen, the resulting product should be 18 grams of water, which is the theoretical yield.
• Loss of product during the process can also contribute to a lower actual yield.
• Actual yield is the amount of product that is obtained after a chemical reaction, which may be less than the expected yield due to factors such as unreacted reactants, side reactions, and loss of product during the process.
• Side reactions are another common reason for not obtaining the expected yield, as the reactants might react to produce a different product than the one that was expected.
• Gaseous products can float off and escape, for example, or if a liquid product is filtered, not all of it may be captured.
• Unreacted reactants are a common reason for not obtaining the expected yield, as some of the mixture may still be reactants at the end of the reaction.