Limiting Reactants and Percent Yield Practice

Front

What is a limiting reactant?

Back

The limiting reactant is the substance that is completely consumed in a chemical reaction, limiting the amount of product that can be formed.

Front

How do you identify the limiting reactant in a reaction?

Back

To identify the limiting reactant, compare the mole ratio of the reactants used in the reaction to the mole ratio from the balanced equation.

Front

What is percent yield?

Back

Percent yield is a measure of the efficiency of a reaction, calculated as (actual yield / theoretical yield) x 100%.

Front

What is the theoretical yield?

Back

The theoretical yield is the maximum amount of product that can be produced from a given amount of reactants, based on stoichiometric calculations.

Front

What is the actual yield?

Back

The actual yield is the amount of product that is actually obtained from a chemical reaction.

Front

In the reaction 1 Mg + 2 HCl ⟶ 1 MgCl2 + 1 H2, if you have 6.00 moles of HCl and 5.00 moles of Mg, which is the limiting reactant?

Back

HCl is the limiting reactant.

Front

In the reaction CuCl2 + 2NaNO3 ⟶ Cu(NO3)2 + 2NaCl, if 15.0 grams of CuCl2 react with 20.0 g of NaNO3, what mass of NaCl is produced?

Back

13.0 g of NaCl.

Front

In the reaction 4NH3 + 5O2 ⟶ 4NO + 6H2O, how many grams of NO are formed from 6.30 g of ammonia and 1.80 g of oxygen?

Back

1.35 g of NO.

Front

In the reaction 4NH3 + 6NO ⟶ 5N2 + 6H2O, what mass of nitrogen gas is produced from 9.00 moles of NH3 and 27.0 moles of NO?

Back

315 g of N2.

Front

In the combustion reaction C3H8 + 5O2 ⟶ 3CO2 + 4H2O, what mass of carbon dioxide is produced from 3.0 g of propane and 2.1 g of oxygen?

Back

0.55 g of CO2.