24 7. Aqueous silver nitrate reacts with solid aluminum to produce aqueous aluminum nitrate and solid silver. If 0.95 moles of solid silver are produced, how many moles of aluminum were reacted?
24 7. Aqueous silver nitrate reacts with solid aluminum to produce aqueous aluminum nitrate and solid silver. If 0.95 moles of solid silver are produced, how many moles of aluminum were reacted?
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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Hi sorry to bother I know that you guys can only answer 3 questions per the ask questions so I was wondering if you could solve the following 3 for me please thank you
![**Stoichiometry**
**Example Problem:**
7. Aqueous silver nitrate reacts with solid aluminum to produce aqueous aluminum nitrate and solid silver. If 0.95 moles of solid silver are produced, how many moles of aluminum were reacted?
**Explanation:**
When dealing with this type of chemical reaction, the stoichiometry of the balanced chemical equation will help in determining the moles of reactants and products.
If we consider the following balanced equation:
\[3 \text{AgNO}_3(aq) + \text{Al(s)} \rightarrow \text{Al(NO}_3\text{)}_3(aq) + 3 \text{Ag(s)}\]
According to the balanced equation:
- 3 moles of silver nitrate react with 1 mole of aluminum to produce 3 moles of silver.
Given:
- 0.95 moles of solid silver are produced.
Using stoichiometry:
\[ \text{Moles of aluminum} = \frac{\text{Moles of silver}}{3} \]
Thus:
\[ \text{Moles of aluminum} = \frac{0.95}{3} \approx 0.317 \text{ moles of aluminum} \]
Therefore, 0.317 moles of aluminum were reacted to produce 0.95 moles of solid silver.
This type of stoichiometry problem is crucial in understanding chemical equations and determining the amount of reactants needed or products formed in a given chemical reaction.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7c430cc2-4097-4d45-9871-f052d1dcc428%2F5129f075-de36-46a4-92da-b8b46e39c631%2F59ejg7f_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Stoichiometry**
**Example Problem:**
7. Aqueous silver nitrate reacts with solid aluminum to produce aqueous aluminum nitrate and solid silver. If 0.95 moles of solid silver are produced, how many moles of aluminum were reacted?
**Explanation:**
When dealing with this type of chemical reaction, the stoichiometry of the balanced chemical equation will help in determining the moles of reactants and products.
If we consider the following balanced equation:
\[3 \text{AgNO}_3(aq) + \text{Al(s)} \rightarrow \text{Al(NO}_3\text{)}_3(aq) + 3 \text{Ag(s)}\]
According to the balanced equation:
- 3 moles of silver nitrate react with 1 mole of aluminum to produce 3 moles of silver.
Given:
- 0.95 moles of solid silver are produced.
Using stoichiometry:
\[ \text{Moles of aluminum} = \frac{\text{Moles of silver}}{3} \]
Thus:
\[ \text{Moles of aluminum} = \frac{0.95}{3} \approx 0.317 \text{ moles of aluminum} \]
Therefore, 0.317 moles of aluminum were reacted to produce 0.95 moles of solid silver.
This type of stoichiometry problem is crucial in understanding chemical equations and determining the amount of reactants needed or products formed in a given chemical reaction.
Transcribed Image Text:Certainly! Below is the transcription of the text for an educational website:
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### Chemistry Problems
2. Methane gas (CH₄) burns in diatomic oxygen gas to produce carbon dioxide gas and water vapor. If 9.5 grams of methane are burned in 45 grams of oxygen, what mass of carbon dioxide is produced?
3. Aqueous copper (II) sulfate reacts with solid zinc to produce aqueous zinc sulfate and solid copper. What mass of copper is produced when 0.0075 moles of copper (II) sulfate reacts with 0.015 moles of zinc?
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In this transcription, problems involving combustion reactions and chemical stoichiometry are posed. The combustion of methane and the single replacement reaction between copper sulfate and zinc are classic exercises to illustrate the principles of mass conservation and mole ratios in balanced chemical equations.
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