Stoichiometry

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

• Write a Balanced Equation
• Panic
• Write an Unbalanced Equation
• Ask for help

Tags

NGSS.HS-PS1-7

 The equation for Percent Yield:

• (predicted/experimental) X 100
• (experimental/predicted) X 100
• (experimental - predicted)/ Predicted X 100

2H₂  +   O₂  →  2H₂O
How many moles of oxygen are consumed if 8 moles H₂ are used?

• 2
• 4
• 6
• 8

Tags

NGSS.HS-PS1-7

What is a Excess Reagent?

• amount you end with
• what you run out of first
• what you have left over
• what you start with

Tags

NGSS.HS-PS1-7

If you predicted that 1.5 moles of Magnessium are used in a reaction, and you have 2.0 moles of Magnessium, what type of reactant is Magnessium?

• Limiting Reactant
• Excess Reactant
• Fast Reacter
• Non-Reactant

Tags

NGSS.HS-PS1-7

If you predicted that 1.5 moles of Magnesium are used in a reaction, and you have 1.0 mole of Magnesium, how much Magnesium is in Excess?

• 0.5 moles Mg
• 1.5 moles Mg
• 1.0 mole Mg
• 0.0 Moles Mg

Tags

NGSS.HS-PS1-7

If a chemist calculates the maximum amount of product that could be obtained in a chemical reaction, he or she is calculating the

• theoretical yield
• mole ratio
• actual yield
• percentage yield

Tags

NGSS.HS-PS1-7

2Na + 2H₂O → 2NaOH+ H₂
How many grams of hydrogen are produced if 120 g of Na are available?

• 5.2 g
• 2.6 g
• 690 g
• 45 g

Tags

NGSS.HS-PS1-7

2 KClO₃ → 2 KCl + 3 O₂
How many moles of oxygen are produced when 6.7 moles of KClO₃ decompose completely?

• 6.7 mol
• 1.0 mol
• 10.1 mol
• 4.5 mol

Tags

NGSS.HS-PS1-7

 SiO₂ + 3C → SiC + 2CO
I need to add 8 moles of Carbon to the reaction. How many grams of Carbon should I weigh?

• _{96 g}
• 0.67 g
• 2.67 g
• 48 g

Tags

NGSS.HS-PS1-7