Chemistry Stoichiometry Worksheet 2-26-09
1. Salt (sodium chloride) is prepared by the reaction of sodium metal with chlorine
gas. Write the balanced equation for this reaction.
2. You have 71.68 L of chlorine and 6.7 moles of sodium. What is the limiting
reagent?
3. What is the excess reagent and how many grams of excess reagent is left?
4. What is the maximum amount number of grams of salt that can be produced in
this reaction?
**Calculate the % yield in each of the following:
5. theoretical yield is 50g of product; actual yield is 41.9g
6. theoretical yield is 290kg of product; actual yield is 270 kg
7. theoretical yield is 6.05 x 10^4kg; actual yield is 4.18 x 10^4kg
8. theoretical yield is .00192g; actual yield is .000089g
9. In commercial production of the element arsenic, arsenic III oxide is heated with
carbon which reduces the oxide to the metal according to the following
SKELETON equation: As2O3 + C CO2 + As
a. write the balanced equation for this reaction
b. if 8.87g of arsenic III oxide is used in the reaction and 5.33g of arsenic is
actually produced what is the theoretical yield?
c. What is the % yield of arsenic in this reaction?
10. Chlorobenzen C6H5Cl is used in the production of many important chemicals
such as aspirin, dyes and disinfectants. One industrial method of preparing
chlorobenzene is to react benzene C6H6 with chlorine to get chlorobenzene and
hydrochloric acid as products. Write the balanced equation for this reaction.
11. When 36.8g of benzene reacts with chlorine the actual yield of chlorobenzene is
38.8g. What is the theoretical yield of chlorobenzene?
12. What is the % yield of chlorobenzene?