Stoichiometry Practice

Molar masses are determined from

• the mole ratio of a given amount of reactant to an unknown amount of product
• the periodic table
• any mole ratio in the equation
• a conversion factor

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NGSS.HS-PS1-7

The limiting reactant

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

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NGSS.HS-PS1-7

What is the theoretical yield?

• the maximum amount of product from a reaction
• the amount of product recovered from a lab experiment
• amount of product that causes the reaction to stop
• the amount of product needed to reverse the reaction

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NGSS.HS-PS1-7

NGSS.HS-PS1-6

N₂ +  3H₂ −->  2NH₃ 
How many moles of ammonium are produced when 3 moles of nitrogen react with hydrogen?

• 6 moles Ammonium
• 1.5 moles ammonium
• 9 moles ammonium
• 9 moles hydrogen

Tags

NGSS.HS-PS1-7

Mole ratios are obtained from the

• balanced chemical equation
• periodic table
• molar mass

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NGSS.HS-PS1-7

Considering the UNBALANCED reaction: 
Fe₂O₃(s) + CO(g) --> Fe(m) + CO₂(g)
If 32 moles of iron metal was produced during the reaction, how many moles of carbon monoxide were consumed?

• 21 moles
• 21.3 moles
• 48 moles
• 64 moles

Tags

NGSS.HS-PS1-7

How many grams are in 1.5 moles of O?

• 9.03 x 10²³ grams
• 16 grams
• 24 grams
• 6.02 x 10²³ grams

How many moles is 4 grams of Calcium?

• 0.10 moles
• 10 moles
• 44 moles
• 160 moles

How many moles are in 6x10²² particles of CO₂?

• 0.1 moles
• 4.4 moles
• 10 moles
• 264 moles

2CO  +  O₂  −-> 2CO₂
How many liters of carbon dioxide are produced from 10L of carbon monoxide?

• 10
• 20
• 1
• 5

Tags

NGSS.HS-PS1-7