University:
High School
Course:
High School Chemistry
Academic year:

2022
Views:

466

Pages:

2
Author:

Nabila N.

Name:_____________________ Per:_____ 49er Worksheet Directions: show all your work, box your answer, and use significant figures to receive credit. 1. Write the pathway to solve a mass to mass stoichiometry problem. 2. Given the unbalanced reaction: ___Fe(s) + ___Cl2(g)  ___FeCl3(s) What mass of chlorine needs to be purchased to use up 25.7 grams of iron? 3. Given the unbalanced reaction: ___CH4(g) + ___O2(g)  ___CO2(g) + ___H2O(g) If 60.0 grams of carbon dioxide are produced, how many grams of steam (H2O gas) are also produced? 4. Given the unbalanced reaction: ___NaClO3(s)  ___NaCl(s) + ___O2(g) If 109 grams of sodium chlorate breakdown, what mass of oxygen will be produced? 5. Given the unbalanced reaction: ___Al(s) + ___O2(g)  ___Al2O3(s) What mass of oxygen is needed to react with 55.1g of aluminum? 6. Given the unbalanced reaction: ___C2H2(g) + ___O2(g)  ___CO2(g) + ___H2O(g) When blow torch designers were testing out their new blow torch model they burned 14.5 grams of acetylene (C2H2). How many grams of CO2 should be produced? b. If 30 grams of CO2 were produced during the experimental trial of the blow torch (as described above), would the designers be happy with these results? Explain. Limiting Reactant Problems 1. You go to make peanut butter and jelly sandwiches. You have 4 slices of bread and a brand new container of PB from Costco & 2 full containers of jelly. a. What is the limiting reactant? Explain. b. How many whole sandwiches can be produced? 2. During photosynthesis, plants produce sugars and oxygen in the following equation: 6 CO2 (g) + 6 H2O (l)  C6H12O6 (s) + 6 O2 (g) a. If 11 g of CO2 is mixed with 5 g of H2O during photosynthesis, how much O2 will the plant be able to produce? (yes, you must do 2 stoichiometry problems) b. Based on your calculations above, which reactant (water or carbon dioxide) will limit how much oxygen can be produced? Explain. 3. ___ Al + __Cl2  __AlCl3 a. Determine the mass in grams of product formed if 15.0 g of Al reacts with 40.0 g of Cl2. b. Identify the limiting reactant. c. If you made 50.0 g of AlCl3 in the lab, what is your percent yield? 4. ___ Fe + __O2  __Fe2O3 a. What is the mass in grams of Fe2O3 produced when 13.0 g of O2 is mixed with 12.2 g of Fe, b. What is the limiting reactant? c. What mass in grams of excess reactant remains when the reaction is complete? d. Kelly performed this reaction in the lab and made 14 grams of Fe2O3, what is her percent yield?