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At high temperatures, sulfur combines with iron to form the brown-black iron (II) sulfide: Fe (s) + S (l)  FeS (s) In one experiment, 7.62 g of Fe are.

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Presentation on theme: "At high temperatures, sulfur combines with iron to form the brown-black iron (II) sulfide: Fe (s) + S (l)  FeS (s) In one experiment, 7.62 g of Fe are."— Presentation transcript:

1 At high temperatures, sulfur combines with iron to form the brown-black iron (II) sulfide: Fe (s) + S (l)  FeS (s) In one experiment, 7.62 g of Fe are allowed to react with 8.67 g of S. What is the limiting reagent, and what is the reactant in excess? Calculate the mass of FeS formed.

2 If a student goes to lab with these amounts of Fe and S and retrieves g of FeS in the lab, what is her percentage yield?

3 What mass of excess reagent remains after the experiment is complete?

4 Acrylonitrile, C 3 H 3 N, is the starting material for the production of a kind of synthetic fiber acrylics) and can be made from propylene, C 3 H 6, by reaction with nitric oxide, NO, as follows: C 3 H 6 (g) + NO (g) → C 3 H 3 N (s) + H 2 O (l) + N 2 (g) What mass of C 3 H 3 N can be made when 21.6 g of C 3 H 6 react with 21.6 g of nitric oxide?

5 When a student carried out this experiment, using the given amounts, he isolated 22.4 g of C 3 H 3 N in lab. What was his percentage yield?

6 What mass of excess reagent remains after the experiment is complete?

7 Formic acid, HCHO 2, burns in oxygen to form carbon dioxide and water as follows: HCHO 2 (aq) + O 2 (g) → CO 2 (g) + H 2 O (l). If a 3.15-g sample of formic acid was burned in 2.0 L of oxygen, what volume of carbon dioxide would be produced? (Assume the reaction occurs at standard temperature and pressure, STP.)

8 Carrying out this experiment, a student was able to retrieve 1.38 L of CO 2 in lab. What was the percentage yield?

9 What mass of excess reagent remains after the experiment is complete?


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