Chapter 9 Test Review

In the chemical reaction described by the equation 4Fe(s) + 3O2(g) → 2Fe2O3(s), the mole ratio of iron(III) oxide to Oxygen is

• 1:1.

• 1:2 or 2:4

• 2:3.

• 4:1.

Molar masses are determined from

• the mole ratio of a given amount of reactant to an unknown amount of product.
• the periodic table.
• any mole ratio in the problem.
• a conversion factor.

The type of stoichiometry problem that involves the least steps is a

• mole-mole conversion.

• mole-to-mass conversion.

• mass-to-mole conversion.

• mass-to-mass conversion.

If, in the reaction A + B → C + D, the quantity of B does not react with all of A,

• A is the limiting reactant.

• B is the excess.

• C is in excess.

• A is in excess.

2As2O3 + 3C → 3CO2 + 4As If 6.0 mol of each reactant are available for the above reaction, the product remaining after the reaction should contain (Hint: You will do two mol-mol problems.)

• 4.0 mol C.
• 4.0 mol CO2.
• 6.0 mol CO2.
• equal quantities of the products.

2As2O3 + 3C → 3CO2 + 4As If 6.0 mol As2O3 reacts with excess carbon, the theoretical yield of the above reaction is

• 32 mol As.

• 12 mol As.

• 8 mol As.

• 4 mol As.

The amount of product a student measures in an experiment is the

• percentage yield.
• theoretical yield.
• actual yield.
• mole ratio.

For the reaction 2H2 + O2 → 2H2O, how many moles of water can be produced from 4.0 mol of oxygen?

• 6.0 mol H2O

• 2.0 mol H2O

• 8 mol H2O

• 3.0 mol H2O

For the reaction 2Na + Cl2 → 2NaCl, how many grams of chlorine gas are required to react completely with 3.00 mol of sodium?

• 106.2 g Cl2

• 35.5 g Cl2

• 280 g Cl2

• 22.9 g Cl2

Given the reaction represented by the following unbalanced equation: N2O(g) + O2(g) → NO2(g) What is the mole ratio of NO2 to N2O?

• 2:3

• 3:4

• 4:3

• 4:2 or 2:1