Chem 2nd Sem Final Review 1

Determine the amount of moles of BaCl₂ that are in 436 g of the compound.

• 3.5 mol

• 2.1 mol

• 4.6 mol

• 2.7 mol

In EXOTHERMIC reactions, energy is _____ from the reaction to the surroundings.

• Absorbed

• Released

• Eliminated

• Evaporated

In ENDOTHERMIC reactions, energy is _____ by the reaction system from the surroundings.

• Absorbed

• Released

• Eliminated

• Obliterated

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

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

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

 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

A chemist interested in the efficiency of a chemical reaction would calculate the

• mole ratio
• rate of reaction
• percent yield
• energy released

What is a Excess Reagent?

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

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