percentage yeild

    Cards (20)

    • What is the term used to describe the amount of product obtained from a chemical reaction?
      Yield
    • How can yield be measured in chemistry?
      In grams or moles
    • What does the term 'actual yield' refer to?
      The amount of product actually obtained from a reaction
    • What does 'theoretical yield' represent?
      The yield expected 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 a reversible reaction?
      A reaction where products can revert back to reactants
    • In the nitrogen and hydrogen reaction to make ammonia, why might we not get the expected amount of ammonia?

      Some ammonia might break back down into nitrogen and hydrogen
    • What are side reactions in a chemical reaction?
      Reactions where reactants produce different products than expected
    • If nitrogen reacts with oxygen instead of hydrogen, what product is formed?
      Nitrogen dioxide
    • What is one way product loss can occur during a reaction?
      Gaseous products can escape into the air
    • What happens when filtering a solution?
      Some liquid or solid may be left behind
    • How do you calculate the percentage yield?
      Divide the actual yield by the 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 does a percentage yield of 100% indicate?
      All predicted products were obtained
    • What is the theoretical yield of the reaction between 2 grams of hydrogen and 16 grams of oxygen?
      18 grams
    • What does a percentage yield of 0% indicate?
      No product was obtained
    • What are the common reasons for a lower actual yield in chemical reactions?
      • Reactants may not fully react
      • Side reactions producing unexpected products
      • Loss of product during the process
    • How do you find the percentage yield from a chemical reaction?
      1. Take the actual yield
      2. Divide by the theoretical yield
      3. Multiply by 100
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