stoich final

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

• 1.16%
• 116%
• 85%
• 76%

When reacting Na with Cl₂, we calculated that the theoretical yield should be 13 grams. Our actual yield was 12.5 grams. What is the percent yield?

• 90.4%

• 104%

• 96.15%

• 1.04%

The theoretical yield of a reaction is 237 grams, but the reaction actually yields 26 less grams than expected. What is the percent yield?

• 17.6%

• 82.4%

• 89.0%

• 121.3%

Which of the following describes a limiting reactant?

• The reactant that is not completely consumed during a reaction

• None of this reactant is left over after the reaction take place

• The reactant that is completely consumed during the reaction

• Some of this reaction is left over after the reaction

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. (Ar P=31, Cl = 35.5)

• 78%

• 64%

• 27%

• 33%

How many grams of FeS are formed from 7.62g of Fe reacted with excess S? (Ar Fe=55.9, S=32.1)

• 3.82g

• 7.62g

• 12.0g

• 11.4g

Silver nitrate and sodium phosphate are reacted in equal amounts of 200 g each. How many grams of silver phosphate are produced? 
3AgNO₃  + Na₃(PO₄)  --->  Ag₃(PO₄)  + 3NaNO₃

• 164 g
• 64 g
• 146 g
• 164 moles

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

Identify the limiting reagent when 6.00 g HCl combines with 5.00 g Mg to form MgCl₂.
a.  Mg +  2HCl --> MgCl₂  +  H₂   
b.  a.  Mg +  2HCl --> MgCl₂  +  H₂   

• Mg
• H₂
• MgCl₂
• HCl

• 6:4

• 4:6

• 1:3

• 3:1