Unit 10- Stoichiometry Review

Mole ratios are obtained from the

• balanced chemical equation
• periodic table
• molar mass

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NGSS.HS-PS1-7

theoretical yield is:

• the experimental value

• the calculated amount using the data table

• the calculated amount using stoichiometry

• the same as the limiting reactant

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Select the true statements about limiting reactants.

• is left over after the reaction is complete

• it is completely used up

• controls the amount of product formed

• the reaction stops when it is used up.

actual yield is:

• always less than 100

• the calculated amount using stoichiometry

• the calculated amount using the data table

• the amount of product recovered in the experiment

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

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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

4 Al + 3 O₂ –> 2 Al₂O₃  How much aluminum would be needed to completely react with 45 grams of O₂?

• 1.05 moles
• 3.75 moles
• 1.875 grams
• 1.875 moles

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Given the equation:

2NaClO₃ (s) → 2NaCl (s) + 3O₂ (g)

When 2.00 moles of NaClO₃ react, how many grams of O₂ is produced?

• 56 g of O₂

• 96 g of O₂

• 64 g O₂

• 32 g O₂

2 NaClO₃ (s) → 2NaCl (s) +3 O₂ (g)

How many grams of O₂ will be produced from 12.00 moles of NaClO₃?

• 256 g of O₂

• 576 g of O₂

• 288 g O₂

• 32 g O₂

2H₂ + O₂ → 2H₂O

How many grams of H₂O can be produced from 3.91 g of O₂?

• 1.905

• 4.4

• 2.2

• 1.1

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NGSS.HS-PS1-7