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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![**Problem Description:**
What is the mass in grams of \( \text{H}_2 \) that can be formed from 88.2 grams of \( \text{NH}_3 \) in the following reaction?
\[ 2 \, \text{NH}_3(g) \rightarrow 3 \, \text{H}_2(g) + \text{N}_2(g) \]
**Explanation:**
This problem involves a stoichiometric calculation that requires determining the mass of hydrogen gas (\( \text{H}_2 \)) produced from a given mass of ammonia (\( \text{NH}_3 \)). The balanced chemical equation provided is crucial for understanding the molar relationships between reactants and products.
To find the solution:
1. Calculate the molar mass of \( \text{NH}_3 \).
2. Determine the moles of \( \text{NH}_3 \) available.
3. Use the stoichiometry of the reaction to find the moles of \( \text{H}_2 \) produced.
4. Convert moles of \( \text{H}_2 \) to grams using its molar mass.
This type of calculation is fundamental in chemistry for predicting product formation in chemical reactions.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F70274774-6f46-4808-8916-795560a9e0a1%2Fea33a231-6742-4486-abc9-46e389d355e4%2Fz61nxnd_processed.png&w=3840&q=75)
Transcribed Image Text:**Problem Description:**
What is the mass in grams of \( \text{H}_2 \) that can be formed from 88.2 grams of \( \text{NH}_3 \) in the following reaction?
\[ 2 \, \text{NH}_3(g) \rightarrow 3 \, \text{H}_2(g) + \text{N}_2(g) \]
**Explanation:**
This problem involves a stoichiometric calculation that requires determining the mass of hydrogen gas (\( \text{H}_2 \)) produced from a given mass of ammonia (\( \text{NH}_3 \)). The balanced chemical equation provided is crucial for understanding the molar relationships between reactants and products.
To find the solution:
1. Calculate the molar mass of \( \text{NH}_3 \).
2. Determine the moles of \( \text{NH}_3 \) available.
3. Use the stoichiometry of the reaction to find the moles of \( \text{H}_2 \) produced.
4. Convert moles of \( \text{H}_2 \) to grams using its molar mass.
This type of calculation is fundamental in chemistry for predicting product formation in chemical reactions.
![**Question:**
How many moles of H₂O can be formed from 7.00 × 10²³ molecules of NH₃ from the following equation?
\[ 4 \text{ NH}_3(g) + 5 \text{ O}_2(g) \rightarrow 4 \text{ NO}(g) + 6 \text{ H}_2\text{O}(g) \]
**Explanation:**
This chemical equation represents the reaction between ammonia (NH₃) and oxygen (O₂) to produce nitrogen monoxide (NO) and water (H₂O). The stoichiometric coefficients indicate the mole ratio of the reactants and products involved in the reaction:
- 4 moles of NH₃ react with 5 moles of O₂
- This produces 4 moles of NO and 6 moles of H₂O
Given 7.00 × 10²³ molecules of NH₃, we need to calculate the corresponding moles of H₂O. Using Avogadro's number (6.022 × 10²³ molecules/mol), we can determine the number of moles of NH₃ and then use the mole ratio to find the moles of H₂O produced.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F70274774-6f46-4808-8916-795560a9e0a1%2Fea33a231-6742-4486-abc9-46e389d355e4%2Fcgos5j6_processed.png&w=3840&q=75)
Transcribed Image Text:**Question:**
How many moles of H₂O can be formed from 7.00 × 10²³ molecules of NH₃ from the following equation?
\[ 4 \text{ NH}_3(g) + 5 \text{ O}_2(g) \rightarrow 4 \text{ NO}(g) + 6 \text{ H}_2\text{O}(g) \]
**Explanation:**
This chemical equation represents the reaction between ammonia (NH₃) and oxygen (O₂) to produce nitrogen monoxide (NO) and water (H₂O). The stoichiometric coefficients indicate the mole ratio of the reactants and products involved in the reaction:
- 4 moles of NH₃ react with 5 moles of O₂
- This produces 4 moles of NO and 6 moles of H₂O
Given 7.00 × 10²³ molecules of NH₃, we need to calculate the corresponding moles of H₂O. Using Avogadro's number (6.022 × 10²³ molecules/mol), we can determine the number of moles of NH₃ and then use the mole ratio to find the moles of H₂O produced.
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