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1. Aluminum metal (Al) reacts with sulfur (S) to produce aluminum sulfide (Al2S3) according to this unbalanced chemical equation: Al(s) + S(s) → _Al2S3(s) a. How many moles of Sulfur are needed to react with 3.96moles of Aluminum? b. If there are 9.49moles of Aluminum and unlimited amounts of sulfur, how many moles of Aluminum Sulfide can be produced? c. If there are 3.29 grams of Aluminum and an unlimited amount of sulfur, how many grams of Aluminum Sulfide can be produced?

1. Aluminum metal (Al) reacts with sulfur (S) to produce aluminum sulfide (Al2S3) according to this unbalanced chemical equation: Al(s) + S(s) → _Al2S3(s) a. How many moles of Sulfur are needed to react with 3.96moles of Aluminum? b. If there are 9.49moles of Aluminum and unlimited amounts of sulfur, how many moles of Aluminum Sulfide can be produced? c. If there are 3.29 grams of Aluminum and an unlimited amount of sulfur, how many grams of Aluminum Sulfide can be produced?

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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**Chem 105: Topic 8 Written HW** Name: _______________________ 1. **Aluminum metal (Al) reacts with sulfur (S) to produce aluminum sulfide (Al₂S₃) according to this unbalanced chemical equation:** \_\_\_ Al(s) + \_\_\_ S(s) ➔ \_\_\_ Al₂S₃(s) a. How many moles of Sulfur are needed to react with 3.9 moles of Aluminum? b. If there are 9.49 moles of Aluminum and unlimited amounts of sulfur, how many moles of Aluminum Sulfide can be produced? c. If there are 3.29 grams of Aluminum and an unlimited amount of sulfur, how many grams of Aluminum Sulfide can be produced? d. How many atoms of aluminum will react completely with 1.33 x 10²⁴ atoms of sulfur? 2. **First, lead (II) nitrate (aq) reacts with sodium hydroxide (aq) to form an insoluble precipitate, lead (II) hydroxide and an aqueous solution of sodium nitrate.** a. Write a balanced chemical equation for this scenario with all physical states included. b. How many grams of sodium hydroxide are required to form 51.63 g of lead hydroxide? 3. **A reaction combines 42.5 grams of silver nitrate with 31.0 grams of potassium bromide in the unbalanced equation:** \_\_\_ AgNO₃(aq) + \_\_\_ KBr(aq) ➔ \_\_\_ AgBr(s) + \_\_\_ KNO₃(aq) a. How many grams of Silver Bromide can be produced from just the Silver Nitrate assuming that the Potassium Bromide is in excess? b. How many grams of Silver Bromide can be produced from just the Potassium Bromide assuming that the Silver Nitrate is in excess? c. From the results in both a and b, what is the theoretical yield of Silver Bromide?
Transcribed Image Text:**Chem 105: Topic 8 Written HW** Name: _______________________ 1. **Aluminum metal (Al) reacts with sulfur (S) to produce aluminum sulfide (Al₂S₃) according to this unbalanced chemical equation:** \_\_\_ Al(s) + \_\_\_ S(s) ➔ \_\_\_ Al₂S₃(s) a. How many moles of Sulfur are needed to react with 3.9 moles of Aluminum? b. If there are 9.49 moles of Aluminum and unlimited amounts of sulfur, how many moles of Aluminum Sulfide can be produced? c. If there are 3.29 grams of Aluminum and an unlimited amount of sulfur, how many grams of Aluminum Sulfide can be produced? d. How many atoms of aluminum will react completely with 1.33 x 10²⁴ atoms of sulfur? 2. **First, lead (II) nitrate (aq) reacts with sodium hydroxide (aq) to form an insoluble precipitate, lead (II) hydroxide and an aqueous solution of sodium nitrate.** a. Write a balanced chemical equation for this scenario with all physical states included. b. How many grams of sodium hydroxide are required to form 51.63 g of lead hydroxide? 3. **A reaction combines 42.5 grams of silver nitrate with 31.0 grams of potassium bromide in the unbalanced equation:** \_\_\_ AgNO₃(aq) + \_\_\_ KBr(aq) ➔ \_\_\_ AgBr(s) + \_\_\_ KNO₃(aq) a. How many grams of Silver Bromide can be produced from just the Silver Nitrate assuming that the Potassium Bromide is in excess? b. How many grams of Silver Bromide can be produced from just the Potassium Bromide assuming that the Silver Nitrate is in excess? c. From the results in both a and b, what is the theoretical yield of Silver Bromide?
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