Limiting Reagents and Percent Yield II (CHEM 1405)

Back to Chemistry 1405 Practice Problems

Write and balance the equations, then solve for the required quantity using dimensional analysis.

  1. Magnesium iodide reacts with liquid bromine in a single replacement reaction.

 

a) Which is the excess reactant and how much excess remains from the reaction of 560 g of MgI2 and 360 g of Br2?

 

 

b) What mass of I2 can be formed from the reaction?

 

 

 

 

  1. Nickel (II) reacts with silver nitrate in a single replacement reaction.

 

a) If 22.9 g of nickel and 112 g of silver nitrate are provided, which is limiting?

 

 

b) What mass of nickel (II) nitrate can be produced?

 

 

 

 

  1. Given the following reaction:

a) If 1.60 mol of CS2 reacts with 5.60 mol of oxygen gas, identify the excess reactant. How many moles of the excess reactant remain after the reaction?

 

 

b) How much SO2 can be produced from the reaction?

 

 

c) How much CO2 can be produced from the reaction?

 

 

 

 

Balance the following equations and then solve for the required quantity using dimensional analysis.

  1. Consider the following reaction:

 

a) Calculate the percent yield for a reaction in which 0.38 g of NO2 reacts with excess O3 and 0.36 g of N2O5 is produced.

 

 

b) What mass of N2O5 will result from the reaction of 6.0 mol of NO2 with excess O3 if there is a 61.1% yield in the reaction?

 

 

 

 

  1. In the following equation:

 

a) What is the percent yield if 14.6 g HCl are produced from 30.0 g NaCl and 0.250 mol of H2SO4?

 

 

b) If 25.6 g of NaCl reacts with excess H2SO4 and 12.3 g of Na2SO4 are produced, what is the percent yield?

 

 

 

 

  1. Assume the following hypothetical reaction takes place (already balanced):

 

a) Calculate percent yield when 0.0251 mol of A reacts to form 0.0349 mol of C.

 

 

b) Calculate the percent yield when 189 mol of B reacts to form 39 mol of D.