Chemistry 2 Final Exam

The calculations of quantities in a chemical reaction, based on mole ratios in a balanced equation.

• stoichiometry

• coefficients

• percent yield

• limiting reactant

This is conserved in every ordinary chemical reaction.

• coefficients

• moles

• mass

• stoichiometry

The reactant that determines the amount of product that can be formed in a reaction.

• percent yield

• excess reactant

• limiting reactant

• theoretical yield

The maximum amount of product that could be formed from given amounts of reactants.

• percent yield

• excess reactant

• limiting reactant

• theoretical yield

The reactant that is not completely used up in a reaction.

• percent yield

• excess reactant

• limiting reactant

• theoretical yield

The amount of product formed when a reaction is carried out in the laboratory.

• percent yield

• theoretical yield

• actual yield

• excess reactant

The ratio of the actual yield to the theoretical yield.

• percent yield

• theoretical yield

• actual yield

• limiting reactant

In every balanced chemical equation, each side of the equation has the same number of ____.

• atoms of each element

• molecules

• moles

• coefficients

What are the coefficients that will balance the following skeleton equation? N₂ + H₂ → NH₃

• 1, 1, 1

• 1, 2, 3

• 3, 2, 1

• 1, 3, 2

How many moles of ammonia can be produced from 2.0 moles of each reactant in the equation N₂ + 3 H₂ → 2 NH₃ ?

• 2.0 mol NH₃

• 1.3 mol NH₃

• 4.0 mol NH₃

• 1.0 mol NH₃