Limiting Reagents and percent yield

Front

What is a limiting reagent?

Back

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

Front

How do you identify the limiting reagent in a reaction?

Back

To identify the limiting reagent, calculate the moles of each reactant and determine which one produces the least amount of product based on the stoichiometry of the reaction.

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

How do you calculate theoretical yield?

Back

Theoretical yield is calculated using stoichiometry based on the balanced chemical equation and the amount of limiting reagent.

Front

What is the formula for calculating percent yield?

Back

Percent yield = (actual yield / theoretical yield) x 100%.

Front

In the reaction Mg + 2 HCl → MgCl2 + H2, which reagent is limiting if 6.00 g HCl and 5.00 g Mg are used?

Back

HCl is the limiting reagent.

Front

If 25.0 g of benzene reacts with excess HNO3 and produces 21.4 g of C6H5NO2, what is the percent yield?

Back

The percent yield is 54.29%.

Front

In the reaction 2 Fe2O3 + C → Fe + 3 CO2, if 28 g of carbon is used and the actual yield of CO2 is 181.2 g, what is the percent yield?

Back

The percent yield of CO2 is 58.83%.

Front

What is the theoretical yield of PCl3 when 75.0 g of P4 reacts with excess Cl2?

Back

The theoretical yield of PCl3 is calculated to be 330 g, leading to a percent yield of 33%.

Front

If a scientist expects to produce 12.3 g of product but only collects 10.1 g, what is the percent yield?

Back

The percent yield is 82%.