Name:    Chapter Four Part I Self Quiz

Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.

1.

Ammonia is prepared by reacting nitrogen and hydrogen gases at high temperature according to the unbalanced chemical equation below.

__ N2(g) + __ H2(g) __ NH3(g)

What are the respective coefficients when the equation is balanced with the smallest whole numbers?
 a. 1, 1, 1 b. 1, 3, 1 c. 1, 3, 2 d. 2, 1, 2 e. 2, 3, 2

2.

Metals react with oxygen to give oxides with the general formula MxOy. Write a balanced chemical equation for the reaction of iron with oxygen to yield iron(III) oxide.
 a. Fe(s) + O2(g) → FeO2(s) b. 2 Fe(s) + 3 O2(g) → Fe2O3(s) c. 3 Fe(s) + O2(g) → Fe3O2(s) d. 4 Fe(s) + 3 O2(g) → 2 Fe2O3(s) e. 6 Fe(s) + O2(g) → 2 Fe3O(s)

3.

Aluminum reacts with oxygen to produce aluminum oxide.

4 Al(s) + 3 O2(g) 2 Al2O3(s)

If 5.0 moles of Al react with excess O2, how many moles of Al2O3 can be formed?
 a. 1.0 mol b. 2.0 mol c. 2.5 mol d. 5.0 mol e. 10.0 mol

4.

The compound P4S3 is used in matches. It reacts with oxygen to produce P4O10 and SO2. The unbalanced chemical equation is shown below.

P4S3(s) + O2(g) P4O10(s) + SO2(g)

What mass of O2 will react with 0.641 grams of P4S3?
 a. 0.0466 g b. 0.0932 g c. 0.186 g d. 0.372 g e. 0.746 g

5.

What is a correct method for determining how many grams of oxygen react with 1.00 gram of pentane?

C5H12(g) + 8 O2(g) 5 CO2(g) + 6 H2O(g)
 a. 1.00 g C5H12   = b. 1.00 g C5H12   = c. 1.00 g C5H12   = d. 1.00 g C5H12   = e. 1.00 g C5H12   =

6.

How many moles of Fe2O3(s) can be produced from the reaction of 0.45 mol Fe(s) with 0.30 mol O2(g)?
 a. 0.15 mol b. 0.20 mol c. 0.23 mol d. 0.45 mol e. 0.75 mol

7.

Magnesium reacts with iodine gas at high temperatures to form magnesium iodide. What mass of MgI2 can be produced from the reaction of 4.44 g Mg and 13.4 g I2?
 a. 2.76 g b. 14.7 g c. 16.0 g d. 17.8 g e. 50.8 g

8.

Aspirin is produced by the reaction of salicylic acid (M = 138.1 g/mol) and acetic anhydride (M = 102.1 g/mol).

C7H6O3(s) + C4H6O3(λ) C9H8O4(s) + C2H4O2(λ)

If 2.04 g of C9H8O4 (M = 180.2 g/mol) is produced from the reaction of 3.00 g C7H6O3 and 5.40 g C4H6O3, what is the percent yield?
 a. 14.2% b. 21.4% c. 24.3% d. 52.1% e. 68.0%

9.

Under certain conditions the reaction of ammonia with excess oxygen will produce a 38.2% yield of NO. How many grams of NH3 must be reacted with excess oxygen to yield 17.5 g of NO?

4 NH3(g) + 5 O2(g) 4 NO(g) + 6 H2O(g)
 a. 3.79 g b. 9.93 g c. 26.0 g d. 32.2 g e. 45.8 g

10.

A 4.65 g sample of an oxide of copper, when heated in a stream of hydrogen, produces Cu(s) and 0.585 g H2O. What is formula for the compound?
 a. Cu2O b. CuO c. CuO2 d. Cu2O3 e. Cu3O4