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Limiting Reagent and Percent Yield. Always start with the balanced equation N 2 (g) + 3H 2 (g) → 2NH 3 (g) The mole ratio is 1:3:2 If we have 1 mole of.

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Presentation on theme: "Limiting Reagent and Percent Yield. Always start with the balanced equation N 2 (g) + 3H 2 (g) → 2NH 3 (g) The mole ratio is 1:3:2 If we have 1 mole of."— Presentation transcript:

1 Limiting Reagent and Percent Yield

2 Always start with the balanced equation N 2 (g) + 3H 2 (g) → 2NH 3 (g) The mole ratio is 1:3:2 If we have 1 mole of N 2 and 6 moles of H 2 what is the limiting reagent? What is the excess reagent?

3 Excess reagent – the reactant that is present in more that he required amount for a complete reaction Limiting reagent – the reactant that is completely consumed in a chemical reaction

4 To solve these problems use the mole bridge Remember: – Only moles can cross – Specifically only the original mole can cross – And to cross you need to multiply or divide

5 4Fe + 3O 2 → 2Fe 2 O mol of Iron react with 0.6 mol of oxygen to form iron(III)oxide. How many moles of iron(III)oxide form? You need a 1:1 comparison to decide who crosses! 0.75 mol0.60 mol X mol

6 4Fe + 3O 2 → 2Fe 2 O mol0.60 mol X mol

7 4Fe + 3O 2 → 2Fe 2 O mol0.60 mol X mol

8 Percentage Yield Yield - the quantity of product produced in a chemical reaction IE what you get from the reaction

9 Two kinds of yield: Actual Yield: what is actually produced or what you can measure after the reaction Theoretical yield: the amount you calculate based on the balanced equation

10 4Fe + 3O 2 → 2Fe 2 O g Theoretical Yield? Theoretical Yield M = g/mol g/mol g/mol

11 4Fe + 3O 2 → 2Fe 2 O g Theoretical Yield = g Theoretical Yield M = g/mol g/mol g/mol

12 Percentage Yield The theoretical yield for a reaction is g and the actual Yield is g. What is the %yield?

13 So what? Environment: Chemical waste Is connected to Poor yielding reactions Money


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