Given the reaction, PCl3 + Cl2, PCl5, if 3.00 moles of Cl2 are used, then how many moles of PCl5 are made?
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a.6.00 moles

b.5.00 moles

c.3.00 moles

d.1.00 mole


2.How many atoms are in

5.00 moles of water (H2O)?

a.8.33 x 10−24 atoms

b. 6.02 x 1023 atoms

c. 3.00 x 1024 atoms

d.9.03 x 1024 atoms

3.Given the balanced equation, Fe2O3 + 3 CO, 2 Fe + 3 CO2, what is the molar ratio of CO to CO2?

a.3:3

b. 3:1

c. 3:2

d.1:3

4.Using the equation, 4Fe + 3O2,  2Fe2O3, if 6 moles of oxygen and an excess of iron were available, how many moles of iron (III) oxide would be produced?

a.3 moles

b. 4 moles

c.5 moles

d.6 moles

5.Using the equation, C5H12 + 8O2,  5CO2 + 6H2O, if 2 moles of pentane (C5H12) were supplied, and an unlimited amount of oxygen were available, how many moles of water would be produced?

a.6 moles

b. 8 moles

c.12 moles

d.16 moles

6.How much volume would 2.00 moles of gas take up, under standard temperature and pressure conditions?

a. 11.2 L

b. 22.4 L

c. 33.6 L

d.44.8 L

7.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 MgCl2 that is produced.

a.75.0 g

b.95.1 g

c.99.3 g

d.104 g

8.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 48.6 g of Mg and 36.5 g of HCl are allowed to react, identify the limiting reagent.

a.Mg

b. HCl

c. MgCl2

d. H2

9.The number of moles of the reagent in excess can be used to calculate the moles of the products of the reaction.

a.TRUE

b.FALSE

10.Red mercury (II) oxide decomposes to form mercury metal and oxygen gas according to the following equation: 2HgO (s) , 2Hg (l) + O2 (g). If 3.00 moles of HgO decompose to form 1.25 moles of O2 and 503 g of Hg, what is the percent yield of this reaction?

a.41.6%

b. 62.5%

c.83.3%

d. 96.9%

11.Red mercury (II) oxide decomposes to form mercury metal and oxygen gas according to the following equation: 2HgO (s) ,  Hg (l) + O2 (g). If 3.55 moles of HgO decompose to form 1.54 moles of O2 and 618 g of Hg, what is the percent yield of this reaction?

a.13.2%

b.42.5%

c.56.6%

d.86.5%

12.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 64.06g of sulfur dioxide is given an opportunity to react with an excess of oxygen to produce 75.00 g of sulfur trioxide, what is the percent yield of this reaction?

a.46.83%

b.60.25%

c.75.55%

d.93.68%

13.Percent yield is calculated by the formula, (Actual Yield/Theoretical Yield) x 100%.

a.TRUE

b.FALSE

14.The theoretical yield for a chemical reaction can not be calculated until the reaction is completed.

a.TRUE

b.FALSE

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