What mass of HC1, in grams, is required to react with 0.840 g of Al(OH)3? Al(OH)3 (s) + 3HCl(aq) → AlCl3 (aq) + 3H₂O(l) Mass of HCI- What mass of water, in grams, is produced? Mass of water = g 9
What mass of HC1, in grams, is required to react with 0.840 g of Al(OH)3? Al(OH)3 (s) + 3HCl(aq) → AlCl3 (aq) + 3H₂O(l) Mass of HCI- What mass of water, in grams, is produced? Mass of water = g 9
Chemistry
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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
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![### Chemical Reaction and Mass Calculation
**Problem Statement:**
Determine the mass of HCl (in grams) required to react with 8.840 g of Al(OH)₃, and find out the mass of water produced in this reaction.
**Chemical Equation:**
\[
\text{Al(OH)}_3 (s) + 3\text{HCl} (aq) \rightarrow \text{AlCl}_3 (aq) + 3\text{H}_2\text{O} (\ell)
\]
**Questions:**
1. What mass of HCl is required?
- **Mass of HCl =** [Input required] g
2. What mass of water, in grams, is produced?
- **Mass of water =** [Input required] g
**Explanation:**
This exercise involves stoichiometry, which is the area of chemistry that involves calculating the relative quantities of reactants and products in chemical reactions. Based on the balanced equation above, one mole of aluminum hydroxide reacts with three moles of hydrochloric acid to produce one mole of aluminum chloride and three moles of water.
To solve this problem, you need to perform the following steps:
1. Convert the given mass of Al(OH)₃ to moles.
2. Use the stoichiometric coefficients from the balanced equation to find the moles of HCl and H₂O required/produced.
3. Convert these moles back to grams using their respective molar masses.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2860bcf7-9e8d-460b-a0cf-53a1e326bc6d%2F9d32a35a-8e02-4368-9a87-74fb9da5049c%2Fo3dngc_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Chemical Reaction and Mass Calculation
**Problem Statement:**
Determine the mass of HCl (in grams) required to react with 8.840 g of Al(OH)₃, and find out the mass of water produced in this reaction.
**Chemical Equation:**
\[
\text{Al(OH)}_3 (s) + 3\text{HCl} (aq) \rightarrow \text{AlCl}_3 (aq) + 3\text{H}_2\text{O} (\ell)
\]
**Questions:**
1. What mass of HCl is required?
- **Mass of HCl =** [Input required] g
2. What mass of water, in grams, is produced?
- **Mass of water =** [Input required] g
**Explanation:**
This exercise involves stoichiometry, which is the area of chemistry that involves calculating the relative quantities of reactants and products in chemical reactions. Based on the balanced equation above, one mole of aluminum hydroxide reacts with three moles of hydrochloric acid to produce one mole of aluminum chloride and three moles of water.
To solve this problem, you need to perform the following steps:
1. Convert the given mass of Al(OH)₃ to moles.
2. Use the stoichiometric coefficients from the balanced equation to find the moles of HCl and H₂O required/produced.
3. Convert these moles back to grams using their respective molar masses.
![**Chemical Reaction of Barium Hydride and Water**
Barium hydride reacts with water to produce barium hydroxide and hydrogen gas:
\[ \text{BaH}_2 (s) + 2 \text{H}_2\text{O} (l) \rightarrow \text{Ba(OH)}_2 (aq) + \text{H}_2 (g) \]
In this reaction scenario:
- When 6.389 g of \(\text{BaH}_2\) is combined with 64.000 g of \(\text{H}_2\text{O}\), the reaction proceeds until all the \(\text{BaH}_2\) is consumed.
- The hydrogen gas produced escapes to the environment.
- The final weight of the flask after the reaction is 70.204 g.
- After the water is evaporated, 7.856 g of \(\text{Ba(OH)}_2\) is left behind.
**Calculation Task:**
Determine the mass of water consumed in the reaction:
\[ \_\_\_\_\_\_\_\_\_\_ \text{g} \, \text{H}_2\text{O} \]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2860bcf7-9e8d-460b-a0cf-53a1e326bc6d%2F9d32a35a-8e02-4368-9a87-74fb9da5049c%2Fspouloj_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Chemical Reaction of Barium Hydride and Water**
Barium hydride reacts with water to produce barium hydroxide and hydrogen gas:
\[ \text{BaH}_2 (s) + 2 \text{H}_2\text{O} (l) \rightarrow \text{Ba(OH)}_2 (aq) + \text{H}_2 (g) \]
In this reaction scenario:
- When 6.389 g of \(\text{BaH}_2\) is combined with 64.000 g of \(\text{H}_2\text{O}\), the reaction proceeds until all the \(\text{BaH}_2\) is consumed.
- The hydrogen gas produced escapes to the environment.
- The final weight of the flask after the reaction is 70.204 g.
- After the water is evaporated, 7.856 g of \(\text{Ba(OH)}_2\) is left behind.
**Calculation Task:**
Determine the mass of water consumed in the reaction:
\[ \_\_\_\_\_\_\_\_\_\_ \text{g} \, \text{H}_2\text{O} \]
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