Percentage Yield

• What is the term used to describe the amount of product obtained from a chemical reaction?

  Yield
• How can yield be measured?

  In grams or moles
• What is the difference between actual yield and theoretical yield?

  Actual yield is the amount obtained from the reaction, while theoretical yield is the expected amount based on calculations
• If 2 grams of hydrogen reacts with 16 grams of oxygen, what is the theoretical yield of water?

  18 grams
• Why might the actual yield be less than the theoretical yield?

  There are several reasons, including incomplete reactions, side reactions, and product loss
• What is one reason why a reaction might not go to completion?

  The reactants might not fully react
• What is an example of a reversible reaction mentioned in the material?

  The reaction of nitrogen and hydrogen to make ammonia
• What is a side reaction?

  A reaction where reactants produce a different product than expected
• In the nitrogen and hydrogen reaction, what could nitrogen react with to produce nitrogen dioxide?

  Oxygen from the air
• What is one way product loss can occur during a reaction?

  Gaseous products can escape
• What happens when filtering a solution?

  Some liquid or solid may be left behind
• How do you calculate percentage yield?

  Divide actual yield by theoretical yield and multiply by 100
• If the actual yield is 15 grams and the theoretical yield is 18 grams, what is the percentage yield?

  83.3%
• What is the range of percentage yield?

  From 0% to 100%
• What does a percentage yield of 100% indicate?

  All predicted products were obtained
• What is the significance of the theoretical yield in a chemical reaction?

  It represents the maximum amount of product expected from the reaction
• How do incomplete reactions, side reactions, and product loss affect the yield of a chemical reaction?

  They all contribute to a lower actual yield compared to the theoretical yield