1. % Yield

2. % yield = actual yield _ x 100 theoretical yield Actual yield is found in a lab or you must be given this value Theoretical yield is amount of product found when you convert your limiting reactant to the product.

3. % Yield 3H 2 + N 2  2NH 3 What is the % yield if you start with 6.00 g of hydrogen and 5.00 grams of nitrogen and you make 2.24 g of ammonia? First, find the limiting reactant. Second, find the theoretical yield by converting the limiting reactant to the product. Third, calculate the % yield using the formula.

4. % Yield 3H 2 + N 2  2NH 3 If you want to actually make 25 grams of ammonia and you know the % yield of the reaction, how much nitrogen would you need to begin with?