Stoichiometry

What is the mole ratio of H₂O to H₃PO₄ in the following chemical equation?   P₄O₁₀ + 6 H₂O --> 4 H₃PO₄ 

• 6:4

• 4:6

• 1:3

• 3:1

Using the following equation:
Fe₂O₃(s) + 3H₂(g) → 2Fe(s) + 3H₂O(l)
How many moles of iron can be made from  6 moles H₂?

• 2 moles

• 4 moles

• 6 moles

• 9 moles

Tags

NGSS.HS-PS1-7

2Al + 3H₂SO₄ -> Al₂(SO₄)₃ + 3H₂
How many grams of aluminum sulfate would be formed if 250g H₂SO₄ completely reacted with aluminum?

• 290 g

• 0.85 g

• 450 g

• 870 g

CH₄  +  2O₂  →  CO₂  +  2H₂O
24 grams of CH₄ was added to the above reaction. Calculate the theoretical yield of CO₂.

• 66 grams

• 33 grams

• 130 grams

• 8.7 grams

Tags

NGSS.HS-PS1-7

The ______________ yield is the maximum amount of product possible in a reaction. This determines the amount of product that should be produced in a perfect setting

• stoichiometry

• theoretical

• actual

• excess

When reacting Na with Cl₂, we calculated that the theoretical yield should be 13.0 grams. Our actual yield was 12.5 grams. What is the percent yield?

• 
  90.4%

• 
  96.2%

• 
  104%

• 1.04%

Tags

NGSS.HS-PS1-7

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%

• 27%

• 64%

• 33%

Tags

NGSS.HS-PS1-7

The reaction of 25.0 g benzene, C₆H₆, with excess HNO₃ resulted in 21.4 g C₆H₅NO₂. What is the percentage yield?

C₆H₆ + HNO₃ → C₆H₅NO₂ + H₂O

• 
  85.6%

• 27.4%

• 54.3%

• 100%

Tags

NGSS.HS-PS1-7

What is a limiting reactant?

• 
  the reactant that determines how much product can be made

• the product that you can make the most of

• the reactant that has leftovers

• the amount of reactants that react with each other

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

• water

• carbon dioxide

• C₁₀H₈