Limited Reagent and Percent Yield

Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.

• 1.16%
• 116%
• 85%
• 76%

When 12 moles of O₂ reacts with 1.1 mole of C₁₀H₈ what is the limiting reactant?  C₁₀H₈ + 12 O₂ --> 10 CO₂ + 4 H₂O

• Oxygen
• C₁₀H₈
• Water
• Carbon Dioxide

Tags

NGSS.HS-PS1-7

4NH₃ + 5O₂ --> 4NO + 6H₂O
How many grams of NO are formed if 6.30g of ammonia react with 1.80g of oxygen? 

• 0.37g
• 0.045g
• 1.35g
• 11.1g

Tags

NGSS.HS-PS1-7

SO₂ + PCl₅ --> SOCl₂ + POCl₃
How much SOCl₂ is produced when 16.2g SO₂ react with 13.7g PCl_5? 

• 7.87g
• 30.1g
• 26.4g
• 19.8g 

Tags

NGSS.HS-PS1-7

When does a chemical reaction stop?

• When the lab is finished
• When the excess reactant is used up
• When the limiting reactant is used up
• Chemical reactions never stop

P₄ + 6Cl₂ --> 4PCl₃ 
The reaction of 75.0g P₄ with excess chlorine gas produces 110g PCl₃ in lab. Find the theoretical yield and calculate percent yield for the reaction. 

• 78%
• 64%
• 27%
• 33%

Tags

NGSS.HS-PS1-7

Using the reaction below, determine the percent yield of H₂ if you reacted 36.0 g of water with excess iron. The actual yield is 3.60 g H₂.
3Fe +  4H₂O → Fe₃O₄ + 4 H₂

• 112%
• 89.1%
• 49.9%
• 0.891%

Tags

NGSS.HS-PS1-7

A reaction was predicted to produce 32.4 grams of a compound. When the product was measured, there were only 26.1 grams made. What is the percent yield?

• 80.6%
• 6.3%
• 24.1%
• 58.5%

Tags

NGSS.HS-PS1-7

The ____________ is the ratio of the actual yield to the theoretical yield that demonstrates the efficiency of the reaction.

• theoretical yield
• percent yield
• actual yield
• product

The limiting reactant

• slows the reaction down
• is used up first
• is the reactant that is left over
• controls the speed of the reaction