CHEM 24112 Lecture Notes - Lecture 29: Titanium Tetrachloride, Lithium Nitride, Nitride
29 Jun 2018
School
Department
Course
Professor
CHEMISTRY 112 – DAY 29 Chapter 9: Section 6
3/30/18
PERCENT YIELD
EXAMPLE 1: Lithium nitride is prepared by the reaction of lithium metal and nitrogen gas. Calculate the mass
of lithium nitride formed from 56.0 g of nitrogen gas and 56.0 g of lithium in the unbalanced equation: Li + N2
Li3N
EXAMPLE 2: Now, suppose in Example 1 that you only got 17.2 g from the reaction. What is your percent
yield?
Theoretical yield: amount of product one would expect to produce based on the amount of limiting reactant
Actual yield: amount of product actually obtained
Percent yield = x 100
EXAMPLE 3: You run a reaction that is supposed to yield 15.0 g of NH3. At the end, you only yield 8.2 g of NH3.
What is your percent yield?
EXAMPLE 4: Methanol can be produced by the following reaction: CO + 2H2 CH3OH. Suppose 68.5 kg of CO
is reacted with 8.60 kg of H2.
a) Calculate the theoretical yield of methanol.
b) If 3.57 x 104 g of methanol is actually produced, what is the percent yield of methanol?
find more resources at oneclass.com
find more resources at oneclass.com
Document Summary
Example 1: lithium nitride is prepared by the reaction of lithium metal and nitrogen gas. Calculate the mass of lithium nitride formed from 56. 0 g of nitrogen gas and 56. 0 g of lithium in the unbalanced equation: li + n 2. Example 2: now, suppose in example 1 that you only got 17. 2 g from the reaction. Theoretical yield: amount of product one would expect to produce based on the amount of limiting reactant. Example 3: you run a reaction that is supposed to yield 15. 0 g of nh 3. At the end, you only yield 8. 2 g of nh3. Example 4: methanol can be produced by the following reaction: co + 2h 2 ch3oh. Suppose 68. 5 kg of co is reacted with 8. 60 kg of h2. a) Example 5: balance the following equation ticl4 + o2 tio2 + cl2: suppose 6. 71 x 103 g of titanium(iv) chloride is reacted with 2. 45 x 103 g of oxygen.
