22. Solid aluminum oxide, AI,O, when combined with water, forms aluminum hydroxide, Al(OH),. Al,0, + 3 H,0 → 2 Al(OH), In one particular reaction, 10.2 grams of Al,O, combine with 1.80 grams of water. Which of these statements is true? a. The aluminum oxide is the limiting reactant b. 0.200 mole of aluminum hydroxide will form c. There will be leftover aluminum oxide at the end of the reaction d. Exactly two moles of aluminum hydroxide will form for each mole of water molecules that react
22. Solid aluminum oxide, AI,O, when combined with water, forms aluminum hydroxide, Al(OH),. Al,0, + 3 H,0 → 2 Al(OH), In one particular reaction, 10.2 grams of Al,O, combine with 1.80 grams of water. Which of these statements is true? a. The aluminum oxide is the limiting reactant b. 0.200 mole of aluminum hydroxide will form c. There will be leftover aluminum oxide at the end of the reaction d. Exactly two moles of aluminum hydroxide will form for each mole of water molecules that react
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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![### Chemical Reaction of Aluminum Oxide with Water to Form Aluminum Hydroxide
**Problem Statement:**
Solid aluminum oxide, Al₂O₃, when combined with water, forms aluminum hydroxide, Al(OH)₃.
\[ \text{Al}_2\text{O}_3 + 3\text{H}_2\text{O} \rightarrow 2\text{Al(OH)}_3 \]
In one particular reaction, 10.2 grams of Al₂O₃ combine with 1.80 grams of water. Which of these statements is true?
1. The aluminum oxide is the limiting reactant.
2. 0.200 mole of aluminum hydroxide will form.
3. There will be leftover aluminum oxide at the end of the reaction.
4. Exactly two moles of aluminum hydroxide will form for each mole of water molecules that react.
**Options Explained:**
- **Option a: The aluminum oxide is the limiting reactant**
- The limiting reactant is the substance that is totally consumed when the chemical reaction is complete. In this scenario, if there is less Al₂O₃ relative to H₂O required for the reaction, Al₂O₃ would be the limiting reactant.
- **Option b: 0.200 mole of aluminum hydroxide will form**
- This statement quantifies the amount of Al(OH)₃ produced. Using stoichiometry, this can be determined from the given masses of reactants.
- **Option c: There will be leftover aluminum oxide at the end of the reaction**
- This suggests that not all of the aluminum oxide will fully react, implying that there is more Al₂O₃ present than required by the amount of H₂O available.
- **Option d: Exactly two moles of aluminum hydroxide will form for each mole of water molecules that react**
- This statement pertains to the mole ratio derived from the stoichiometric equation. It suggests the relation between the moles of Al(OH)₃ produced and H₂O used.
For further understanding, one can calculate the number of moles of reactants to determine the limiting reactant and calculate the amount of product formed. This requires converting grams to moles using molecular weights, followed by applying the stoichiometric coefficients from the balanced chemical equation.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7345e8e6-7416-43d6-9fee-55115ecf20af%2Fafa6912f-469c-49d4-881b-a6388a202762%2Ftjqu2qa_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Chemical Reaction of Aluminum Oxide with Water to Form Aluminum Hydroxide
**Problem Statement:**
Solid aluminum oxide, Al₂O₃, when combined with water, forms aluminum hydroxide, Al(OH)₃.
\[ \text{Al}_2\text{O}_3 + 3\text{H}_2\text{O} \rightarrow 2\text{Al(OH)}_3 \]
In one particular reaction, 10.2 grams of Al₂O₃ combine with 1.80 grams of water. Which of these statements is true?
1. The aluminum oxide is the limiting reactant.
2. 0.200 mole of aluminum hydroxide will form.
3. There will be leftover aluminum oxide at the end of the reaction.
4. Exactly two moles of aluminum hydroxide will form for each mole of water molecules that react.
**Options Explained:**
- **Option a: The aluminum oxide is the limiting reactant**
- The limiting reactant is the substance that is totally consumed when the chemical reaction is complete. In this scenario, if there is less Al₂O₃ relative to H₂O required for the reaction, Al₂O₃ would be the limiting reactant.
- **Option b: 0.200 mole of aluminum hydroxide will form**
- This statement quantifies the amount of Al(OH)₃ produced. Using stoichiometry, this can be determined from the given masses of reactants.
- **Option c: There will be leftover aluminum oxide at the end of the reaction**
- This suggests that not all of the aluminum oxide will fully react, implying that there is more Al₂O₃ present than required by the amount of H₂O available.
- **Option d: Exactly two moles of aluminum hydroxide will form for each mole of water molecules that react**
- This statement pertains to the mole ratio derived from the stoichiometric equation. It suggests the relation between the moles of Al(OH)₃ produced and H₂O used.
For further understanding, one can calculate the number of moles of reactants to determine the limiting reactant and calculate the amount of product formed. This requires converting grams to moles using molecular weights, followed by applying the stoichiometric coefficients from the balanced chemical equation.
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