3.3 Yield and atom economy of chemical reactions

    Cards (46)

    • The use of a catalyst can increase the yield of a reaction.

      True
    • The percentage yield is calculated using the formula: Percentage yield = (Actual yield / Theoretical yield) × 100
    • Atom economy focuses on the percentage of reactant mass in the product
    • The ideal value for atom economy is 100%.
      True
    • What effect does an incomplete reaction have on yield?
      Decreases yield
    • Why is the actual yield often less than the theoretical yield?
      Incomplete reactions or losses
    • Atom economy and yield both measure the same aspect of a chemical reaction.
      False
    • What is the focus of atom economy in chemical reactions?
      Efficiency of converting raw materials
    • Stoichiometry is a factor that affects atom economy.

      True
    • What does yield measure in a chemical reaction?
      Amount of product obtained
    • What is the goal in chemistry regarding yield and atom economy?
      Maximize both
    • Theoretical yield is based on the stoichiometry of the balanced equation.
    • Match the yield type with its characteristic:
      Theoretical Yield ↔️ Maximum calculated product
      Actual Yield ↔️ Measured amount of product obtained
    • Atom economy measures how efficiently raw materials are converted into the target compound.

      True
    • What is the formula for calculating atom economy?
      Mass of desired productTotal mass of reactants×100\frac{\text{Mass of desired product}}{\text{Total mass of reactants}} \times 100
    • What is the goal in chemistry regarding yield and atom economy?
      Maximize both
    • How do incomplete reactions affect yield?
      Decrease yield
    • Match the factor with its effect on atom economy:
      Stoichiometry ↔️ Ensures maximum product mass
      Side Reactions ↔️ Reduces atom economy
      Catalyst Use ↔️ Increases atom economy
      Starting Materials ↔️ Optimizes product conversion
    • Match the characteristic with the correct concept:
      Definition ↔️ Percentage of reactant mass in product ||| Actual product amount vs. theoretical maximum
      Focus ↔️ Efficiency of converting raw materials ||| Quantity of product obtained
    • Incomplete reactions and side reactions can decrease the actual yield of a reaction.
    • Catalysts can increase the yield of a reaction.

      True
    • What is the definition of actual yield in a chemical reaction?
      Measured amount of product obtained
    • What is the formula for calculating percentage yield?
      Actual yieldTheoretical yield×100\frac{\text{Actual yield}}{\text{Theoretical yield}} \times 100
    • What is the formula for calculating atom economy?
      Mass of desired productTotal mass of reactants×100\frac{\text{Mass of desired product}}{\text{Total mass of reactants}} \times 100
    • What does atom economy measure?
      Efficiency of raw materials
    • Match the characteristic with the correct term:
      Product amount vs. theoretical maximum ↔️ Yield
      Percentage of reactant mass in product ↔️ Atom Economy
    • The ideal value for both yield and atom economy is 100%.
      True
    • Losses during workup and purification can decrease the final isolated yield.
    • What does maximizing atom economy lead to?
      Less waste
    • What is the theoretical yield of hydrogen gas when 10g of water is electrolyzed according to the equation 2H_{2}O(l) \rightarrow 2H_{2}(g) + O_{2}(g)</latex>?
      1.11 grams
    • To solve GCSE chemistry problems, the first step is to understand the question.
    • Yield in a chemical reaction refers to the amount of product obtained compared to the theoretical maximum
    • The theoretical yield is the maximum amount of product calculated based on the limiting
    • What is atom economy a measure of in a chemical reaction?
      Efficiency
    • What is the definition of atom economy in chemical reactions?
      Percentage of reactant mass in product
    • Atom economy is a measure of the efficiency of a reaction.
    • Atom economy measures the percentage of the total mass of reactants that ends up in the desired product.

      True
    • Order the factors affecting yield from most negative to most positive effect:
      1️⃣ Incomplete reaction
      2️⃣ Side reactions
      3️⃣ Losses during purification
      4️⃣ Optimized reaction conditions
      5️⃣ Catalyst use
    • Side reactions can lower the actual yield of a reaction.

      True
    • If the theoretical yield is 25g and the actual yield is 20g, the percentage yield is 80%.