Final Exam Review 1- 3rd Quarter

For the Balanced Reaction: 3 Mg + 1 Fe₂O₃ → 3 MgO + 2 Fe; What is the Ratio of moles of Mg to moles Fe?

• 3mol Mg / 2 mol Fe
• 2 mol Mg/ 3 mol Fe
• 1 mol Fe/ 2 mol Fe
• 3 mol MgO / 2 mol Fe

Tags

NGSS.HS-PS1-7

How many particles are in a mole?

• 602
• 602 million
• 602 moles
• 6.02 x 10²³

Using the balanced equation in question 1,
Mg(s)   +   HCl(aq)  -->   MgCl₂(aq)   +   H₂(g)
How many grams of HCl are consumed by the reaction of 2.50 moles of magnesium?

• 5.00 g
• 7.29
• 182 g
• 218 g

Tags

NGSS.HS-PS1-7

Fe₂O₃ + 3H₂ → 2Fe + 3H₂O
About how many grams of H₂O will be produced from 150 grams of Fe₂O₃? 

• 50 grams H₂O
• 60 grams H₂O
• 5000 grams H₂O
• 6000 grams H₂O

Tags

NGSS.HS-PS1-7

N₂ +  3H₂ −->  2NH₃ 
How many moles of hydrogen are needed to react with 2 moles of nitrogen?

• 6
• 2
• 3
• 1

N₂ +  3H₂ −->  2NH₃ 
How many moles of hydrogen are needed to react with 2 moles of nitrogen?

• 6
• 2
• 3
• 1

Where are the numbers for a mole ratio found?

• They are part of the chemical formulas for the reactants / products.

• They are given in the problem.

• They are found on the periodic table for those elements.

• They are found as coefficients in the reaction's balanced chemical equation.

Tags

NGSS.HS-PS1-7

Fe (s) + S (l) --> FeS (s)  

In the experiment above, 7.62 g of Fe are allowed to react with 8.67 g of S.
How much FeS is formed?

• 14.8 g
• 12.2 g
• 13.7 g
• 19.9 g

Tags

NGSS.HS-PS1-7

What is a limiting reactant?

• the reactant that determines how much product can be made
• the reactant that is in excess
• the product that you can make the most of
• 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
• C₁₀H₈
• Water
• Carbon Dioxide