Chem 1 Unit 9 Stoichiometry

The limiting reactant determines

• how much product can be made
• how much product can be destroyed
• how much product can be decomposed
• how much product can be eaten

1 H₂SO₄  +  2 NaOH  -->  2 H₂O  +  1 Na₂SO_{4
How many moles of NaOH are needed to react with 1 moles of}  H₂SO₄ ?

• 1 mol NaOH
• 2 mol NaOH
• 3 mol NaOH
• 4 mol NaOH

1 H₂SO₄ +  2 NaOH  -->  2 H₂O  +  1 Na₂SO₄
How many moles of water could be produced from 12 moles of NaOH?

• 2 mol H₂O
• 4 mol H₂O
• 6 mol H₂O
• 12 mol H₂O

How many moles of nitrogen gas are in 135 L of nitrogen gas at Standard Temperature and Pressure (STP)?

• 9.64 moles of N₂

• 5.53 moles of N₂

• 6.02 moles of N₂

• 4.82 moles of N₂

What is the first thing you must do to solve a stoichiometry problem?

• Write a Balanced Equation
• Panic
• Write an Unbalanced Equation
• Avogadro's Number

In the reaction 2 H₂ + O₂ → 2 H₂O what is the mole ratio of oxygen to water?

• 1:2
• 2:1
• 3:4
• 4:3

What is the ratio of the actual yield to the theoretical yield, multiplied by 100%?

• mole ratio

• percentage yield

• Avogadro yield

• excess yield

What is the measured amount of a product obtained from a chemical reaction?

• mole ratio

• percentage yield

• theoretical yield

• actual yield

In a reaction, 9 grams of a substance are produced. The theoretical yield was 10 grams. What is the percentage yield?

• 80%

• 85%

• 90%

• 95%

Determine the mass of calcium hydroxide produced when calcium carbide reacts with 0.64g of water according ot the following equation

CaC₂ + 2H₂O --> Ca(OH)₂ + C₂H₂

• 10.31 g Ca(OH)₂

• 41.31 g Ca(OH)₂

• 1.31 g Ca(OH)₂

• 31 g Ca(OH)₂