# Balanced Equations – Stoichiometry Worksheet – Chemistry

### Stoichiometry Worksheet, Balanced Equations, Grams, Reactant, Limiting Reactant

The key terms in this Chemistry course include Stoichiometry Worksheet, Balanced Equations, Grams, Reactant, Limiting Reactant, Excess Reactant, Product, Reaction, Theoretical yield, Calculations, P4, Cl2, PCl3, H3PO4, Fe2O3,H2O, CO, Fe, CO2, P4O10, Stoichiometry Worksheet – Chemistry.

• Using the three balanced equations below, do 9.a through 9.d for each:
1. How many grams of the first product can be produced from 20.0 grams of the first reactant and 20.0 grams of the second reactant?
2. Which reactant is the limiting reactant?
3. How many grams of the excess reactant are reacted?
4. How many grams of the excess reactant are left unreacted?

P4  + 6Cl2   4PCl3                        P4O10  + 6H2O  4H3PO4        Fe2O3 + 3CO  2Fe+ 3CO2

P4  + 6Cl2   4PCl3

How many grams of the first product can be produced from 20.0 grams of the first reactant and 20.0 grams of the second reactant?

68.71 g 2nd reactant needed.

• A student carried out the reaction shown by reacting 10.0g P4 with excess Cl2 and obtained 35.0g  of PCl3

P4 + 6Cl2   ➡    4PCl3

What is the theoretical yield of PCl3?

Calculate the % yield ofPCl3

##### Calculations

10.      A student carried out the reaction shown by reacting 10.0g P4 with excess Cl2 and obtained 35.0g  of PCl3.

P4 + 6Cl2 4PCl3

Theoretical Yield of PCl3

10 x (1/123.9) x (4/1) x (137.88/1) = 44.51g

% Yield of PCl3

(35/44.51) x 100 = 78.63 %

• Using the three balanced equations below, do 9.a through 9.d for each:
1. How many grams of the first product can be produced from 20.0 grams of the first reactant and 20.0 grams of the second reactant?
2. Which reactant is the limiting reactant?
3. How many grams of the excess reactant are reacted?
4. How many grams of the excess reactant are left unreacted?

P4  + 6Cl2 ➡  4PCl3P4O10  + 6H2O 4H3PO4Fe2O3 + 3CO ➡ 2Fe+ 3CO2

P4  + 6Cl2 ➡  4PCl3

How many grams of the first product can be produced from 20.0 grams of the first reactant and 20.0 grams of the second reactant?

68.71 g 2nd reactant needed.

• A student carried out the reaction shown by reacting 10.0g P4 with excess Cl2 and obtained 35.0g  of PCl3

P4 + 6Cl2   ➡    4PCl3

What is the theoretical yield of PCl3?

Calculate the % yield ofPCl3

##### Calculations

10.      A student carried out the reaction shown by reacting 10.0g P4 with excess Cl2 and obtained 35.0g  of PCl3.

P4 + 6Cl2 4PCl3

Theoretical Yield of PCl3

10 x (1/123.9) x (4/1) x (137.88/1) = 44.51g

% Yield of PCl3

(35/44.51) x 100 = 78.63 %

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