Stoichiometry Review

Knowing the mole ratio of a reactant and product in a chemical reaction would allow you to determine

• the energy released in the reaction.

• the speed of the reaction.

• the mass of the product produced from a known mass of reactant.

• whether the reaction is reversible.

In the equation 6CO₂ + 6H₂O --> C₆H₁₂O₆ +6O₂, the mole ratio of water to oxygen is

• 2:1

• 1:1

• 3:2

• 6:8

In the equation Al₂(SO₄)₃ + 3Ca(OH)₂ --> 3CaSO₄ + 2Al(OH)₃, the mole ratio of calcium hydroxide to aluminum hydroxide is

• 1:3

• 2:3

• 1:1

• 3:2

For the reaction represented by the equation N₂ + 3H₂ --> 2NH₃, how many moles of nitrogen are required to produce 18 mol of ammonia?

• 9

• 18

• 27

• 37

In the reaction represented by the equation A + B --> C + D, if there is more reactant B than is required to completely react with all of A, then

• A is the limiting reactant.

• B is the limiting reactant.

• there is no limiting reactant.

• no product can be formed.

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.

• percentage yield.

• mole ratio.

• actual yield.

The theoretical yield of a chemical reaction is generally

• greater than the actual yield.

• less than the actual yield.

• equal to the percentage yield.

• greater than the percentage yield.

The most steps are required to solve stoichiometry problems when the reactant is given in grams and the product is sought in

• moles.

• grams.

• liters.

• number of atoms.