Question 3

1. Given the reaction, PCl₃ + Cl₂    PCl₅, if 3.00 moles of Cl₂ are used, then how many moles of PCl₅ are made?
3. 6.00 moles
5. 5.00 moles
7. 3.00 moles
9. 1.00 mole

3 points 

Question 4

1. How many moles of a gas are contained in 11.2 liters of a gas, under standard temperature and pressure conditions?
3. 22.4 moles
5. 11.2 moles
7. 1 mole
9. 0.5 moles

3 points 

Question 5

1. How many moles does 22.4 liters of oxygen gas at standard temperature and pressure represent?
3. 1.0 mole
5. 22.4 moles
7. 6.02 x 10²³Â moles
9. 1.30 x 10²⁵ moles

3 points 

Question 6

1. Using the equation, 4Fe + 3O₂  2Fe₂O₃, if 6 moles of iron (III) oxide were produced, how many moles of iron would be required?
3. 4 moles
5. 8 moles
7. 12 moles
9. 16 moles

3 points 

Question 7

1. When magnesium metal and an aqueous solution of hydrochloric acid combine, they produce an aqueous solution of magnesium chloride and hydrogen gas. Using the equation, Mg (s) + 2HCl (aq)   MgCl₂ (aq) + H₂ (g), if 24.3 g of Mg and 75.0 g of HCl are allowed to react, calculate the mass of H₂ that is produced.
3. 1.00 g
5. 2.00 g
7. 4.00 g
9. 5.00 g

3 points 

Question 8

1. When magnesium metal and an aqueous solution of hydrochloric acid combine, they produce an aqueous solution of magnesium chloride and hydrogen gas. Using the equation, Mg (s) + 2HCl (aq)   MgCl₂ (aq) + H₂ (g), if 36.5 g of Mg and 2 moles of HCl are supplied, identify the limiting reagent.
3. Mg
5. HCl
7. MgCl₂
9. H₂

3 points 

Question 9

1. In order to properly calculate which reactant is limiting, the amount of each reactant, in grams, must be compared.
3. TRUE
5. FALSE

2 points 

Question 10

1. Ammonia gas is formed from nitrogen gas and hydrogen gas, according to the following equation: N₂ (g) + 3H₂(g)   2NH₃ (g). If 84.0 g of nitrogen gas is allowed to react with an excess of hydrogen gas to produce 85.0 g of ammonia, what is the percent yield of this reaction?
3. 42.2%
5. 65.0%
7. 70.3%
9. 83.3%

3 points 

Question 11

1. In the manufacturing process of sulfuric acid, sulfur dioxide is reacted with oxygen to produce sulfur trioxide. Using the equation, 2SO₂ (g) + O₂  2SO₃ (g), if 128 g of sulfur dioxide is given the opportunity to react with an excess of oxygen, but only produces 144 g of sulfur trioxide, what is the percent yield of this reaction?
3. 29.24%
5. 58.48%
7. 90.0%
9. 100.0%

3 points 

Question 12

1. Ammonia gas is formed from nitrogen gas and hydrogen gas according to the following equation: N₂ (g) + 3H₂(g)   2NH₃ (g). If 112 grams of nitrogen gas is allowed to react with an excess of hydrogen gas to produce 120 grams of ammonia, what is the percent yield of this reaction?
3. 44.1%
5. 66.2%
7. 88.3%
9. 96.4%

3 points 

Question 13

1. The comparison of the actual yield to the theoretical yield gives an indication of how efficient the reaction is.
3. TRUE
5. FALSE

2 points 

Question 14

1. Once the percent yield has been determined for a reaction, that percent yield will never vary.
3. TRUE
5. FALSE

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Status NEW Posted 19 Jun 2017 03:06 AM My Price 7.00

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