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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?

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?

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
Section: Chapter Questions
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:** \(_\_\_ \, \text{Al}(s) + \_\_\_ \, \text{S}(s) \rightarrow \_\_\_ \, \text{Al}_2\text{S}_3(s)\) a. How many moles of Sulfur are needed to react with 3.96 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 51.63g of lead hydroxide? 3. **A reaction combines 42.5 grams of silver nitrate with 31.0 grams of potassium bromide in the unbalanced equation:** \(\_\_\_ \, \text{AgNO}_3(aq) + \_\_\_ \, \text{KBr}(aq) \rightarrow \_\_\_ \, \text{AgBr}(s) + \_\_\_ \, \text{KNO}_3(aq)\) 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:** \(_\_\_ \, \text{Al}(s) + \_\_\_ \, \text{S}(s) \rightarrow \_\_\_ \, \text{Al}_2\text{S}_3(s)\) a. How many moles of Sulfur are needed to react with 3.96 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 51.63g of lead hydroxide? 3. **A reaction combines 42.5 grams of silver nitrate with 31.0 grams of potassium bromide in the unbalanced equation:** \(\_\_\_ \, \text{AgNO}_3(aq) + \_\_\_ \, \text{KBr}(aq) \rightarrow \_\_\_ \, \text{AgBr}(s) + \_\_\_ \, \text{KNO}_3(aq)\) 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?
Chem 105: Topic 8 Written HW Name: ___________________________ d. *(Problem 3 Continued…)* What reactant led to the theoretical yield of Silver Bromide? What do we call this reactant? e. If a student reported 32.6 grams of the AgBr(s) being produced, what is the percent yield? 4. **Aluminum hydroxide**, one of the antacid ingredients in Maalox, can be prepared by the reaction of aluminum sulfate and sodium hydroxide. How many milliliters of 0.200 M NaOH solution are needed to completely react with 3.50 g of aluminum sulfate? a. Write a balanced chemical equation for the double replacement reaction. Show all physical states. (Remember that your compounds need to be neutral BEFORE balancing or else it will not work). b. How many moles of NaOH are needed to react with 3.50 g of Aluminum Sulfate? c. If the solution of NaOH is 0.200 M, determine how many mL is needed based on your mole amounts in part b. 5. Chalk is composed of calcium carbonate. This water-insoluble compound is formed when a solution of calcium chloride is added to a solution of sodium carbonate. What volume (in mL) of 0.550 M calcium chloride is required to completely react with 750.0 mL of 0.250 M sodium carbonate solution? (You will need to show all steps in this problem.)
Transcribed Image Text:Chem 105: Topic 8 Written HW Name: ___________________________ d. *(Problem 3 Continued…)* What reactant led to the theoretical yield of Silver Bromide? What do we call this reactant? e. If a student reported 32.6 grams of the AgBr(s) being produced, what is the percent yield? 4. **Aluminum hydroxide**, one of the antacid ingredients in Maalox, can be prepared by the reaction of aluminum sulfate and sodium hydroxide. How many milliliters of 0.200 M NaOH solution are needed to completely react with 3.50 g of aluminum sulfate? a. Write a balanced chemical equation for the double replacement reaction. Show all physical states. (Remember that your compounds need to be neutral BEFORE balancing or else it will not work). b. How many moles of NaOH are needed to react with 3.50 g of Aluminum Sulfate? c. If the solution of NaOH is 0.200 M, determine how many mL is needed based on your mole amounts in part b. 5. Chalk is composed of calcium carbonate. This water-insoluble compound is formed when a solution of calcium chloride is added to a solution of sodium carbonate. What volume (in mL) of 0.550 M calcium chloride is required to completely react with 750.0 mL of 0.250 M sodium carbonate solution? (You will need to show all steps in this problem.)
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