1. Unit 7 Limiting Reactants

2. Limiting Reactants

3. Limiting Reactants N2 (g) + 3 H2 (g)  2 NH3 (g) If we start off with 100 moles of N2 and 100 moles of H2, how many moles of NH3 can be produced?

4. Limiting Reactants N2 (g) + 3 H2 (g)  2 NH3 (g) If we start off with 100 moles of N2 and 100 moles of H2:

5. Limiting Reactants N2 (g) + 3 H2 (g)  2 NH3 (g) If we start off with 100 moles of N2 and 100 moles of H2:

6. Limiting Reactants N2 (g) + 3 H2 (g)  2 NH3 (g) If we start off with 100 moles of N2 and 100 moles of H2:

7. Limiting Reactants N2 (g) + 3 H2 (g)  2 NH3 (g) If we start off with 100 moles of N2 and 100 moles of H2, how many moles of NH3 can be produced? How much reactants are left?

8. Limiting Reactants Cu(s) + H2SO4(aq)  CuSO4(aq) + H2O(l) + SO2(g) How much SO2 (in grams) can be produced from 18.00 g of Cu and 18.00 g of H2SO4? How much copper is left over?

9. Limiting Reactants Aluminum oxide can be produced from the following chemical reaction How much Al2O3 can be prepared (in grams) from50.0 g of Al and 100.0 g of O2? 4 Al + 3 O2 2 Al2O3 10.0 g of Al and 10.0 g of O2 11.0 g of Al and 9.40 g of O2

10. Theoretical and Percent Yield Theoretical Yield Maximum amount of a product that can be produced from a given amount of reactants Actual Yield The amount of a product actually obtained from a chemical reaction Percent Yield = Actual Yield Theoretical Yield 4 Al + 3 O2 2 Al2O3 If the Percent Yield is 82%, how much Al2O3 is actually produced? 50.0 g of Al and 100.0 g of O2