After determining the limiting reactant, how do you find the mass of a product?

[Erin Jannusch]

EX. from module 3:
21. According to the following equation, 0.750 g of C6H9Cl3 is mixed with 1.000 kg of AgNO3 in a flask of water. A white solid, AgCl, completely precipitates out. What is the mass of AgCl produced?

C6H9Cl3 + 3AgNO3 ---> AgCl + C6H9(NO3)3.

Molar Mass: C6H9Cl3 (187.50 g/mol), 3AgNO3 (169.88 g/mol), AgCl (143.32 g/mol)

[Jared Smith 1E]

Once you have determined the limiting reactant, you look at the formula and determine how many moles of product can be formed based on the moles of limiting reactant present (the molar ratio of the limiting reactant to the product). Then convert the moles to grams by multiplying by the molar mass.

[Brigitte Phung 1F]

After you determine the limiting reactant, which in this case is C6H9Cl3, you would multiply the moles of C6H9Cl3 by its molar ratio with AgCl, which is 1 mol C6H9Cl3 : 3 mol AgCl (from the balanced equation). This gives you the moles of AgCl produced, which you can then multiply with the molar mass of AgCl (143.32 g/mol) to get the mass of the product.