1. Percent Yield Homework Notes: Thursday, April 7 th, 2016 1

2. 2 Important Vocabulary Theoretical yield The maximum amount of product calculated using the balanced equation. Actual yield The amount of product obtained (what you actually got) when the reaction takes place. Percent yield The ratio of actual yield to theoretical yield. percent yield = actual yield (g) x 100 theoretical yield (g)

3. What is percent yield & why is it important? When we perform stoichiometric calculations to determine the amount of product produced – that is a theoretical yield. But when we actually perform the experiment in a lab setting, we usually find we do not get as much product, we usually get a smaller actual yield. (Human error, amirite?) 3

4. 4 To calculate the percent yield, the actual yield and theoretical yield are needed. You prepared cookie dough to make 5 dozen cookies. The phone rings and you answer. While talking, a sheet of 12 cookies burn and you have to throw them out. The rest of the cookies are okay. What is the percent yield of edible cookies? Theoretical yield 60 cookies possible Actual yield 48 cookies to eat Percent yield 48 cookies x 100 = 80% yield 60 cookies Calculating Percent Yield

5. 5 Learning Check Without proper ventilation and limited oxygen, the reaction of carbon and oxygen produces carbon monoxide. 2C(g) + O 2 (g) 2CO(g) What is the percent yield if 40.0 g CO are actually produced when 30.0 g O 2 are used? (Need to find the theoretical 1 st ) 1) 25.0% 2) 75.0% 3) 76.2%

6. 6 Solution 3) 76.2 % yield theoretical yield of CO 30.0 g O 2 x 1 mol O 2 x 2 mol CO x 28.01 g CO 32.00 g O 2 1 mol O 2 1 mol CO = 52.5 g CO (theoretical) percent yield 40.0 g CO (actual) x 100 = 76.2 % yield 52.5 g CO (theoretical)

7. 7 Learning Check When N 2 and 5.00 g H 2 are mixed, the reaction produces 16.0 g NH 3. What is the percent yield for the reaction? N 2 (g) + 3H 2 (g) 2NH 3 (g) 1) 31.3 % 2) 56.5 % 3) 80.0 %

8. 8 Solution 2) 56.5 % N 2 (g) + 3H 2 (g) 2NH 3 (g) 5.00 g H 2 x 1 mol H 2 x 2 mol NH 3 x 17.03 g NH 3 2.016 g H 2 3 mol H 2 1 mol NH 3 = 28.2 g NH 3 (theoretical) Percent yield = 16.0 g NH 3 x 100 = 56.7 % 28.2 g NH 3