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 and Stoichiometry Problem
**Problem Statement:**
How many grams of NH₃ are needed to completely react with 12.70 g of O₂? Furthermore, how many grams of H₂O would be formed in the reaction?
**Reaction 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 balanced chemical equation represents the reaction between ammonia (NH₃) and oxygen (O₂) to form nitrogen monoxide (NO) and water (H₂O). The coefficients in the equation indicate the molar ratios in which the reactants and products participate in the reaction.
To solve the problem:
1. Convert the mass of O₂ (12.70 g) to moles using its molar mass.
2. Use the mole ratio from the balanced equation to find the moles of NH₃ required.
3. Convert the moles of NH₃ to grams using its molar mass.
4. Use the mole ratio to find the moles of H₂O produced.
5. Convert the moles of H₂O to grams using its molar mass.
This exercise involves understanding stoichiometry, which is fundamental in chemistry for predicting the amounts of substances consumed and produced in a chemical reaction.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F805df41e-b889-4c16-a267-318b4eb3cf21%2Fdb20c0ce-a52c-43e3-af60-0e2983ceee84%2Fuws6hq5_processed.png&w=3840&q=75)
Transcribed Image Text:### Chemical Reaction and Stoichiometry Problem
**Problem Statement:**
How many grams of NH₃ are needed to completely react with 12.70 g of O₂? Furthermore, how many grams of H₂O would be formed in the reaction?
**Reaction 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 balanced chemical equation represents the reaction between ammonia (NH₃) and oxygen (O₂) to form nitrogen monoxide (NO) and water (H₂O). The coefficients in the equation indicate the molar ratios in which the reactants and products participate in the reaction.
To solve the problem:
1. Convert the mass of O₂ (12.70 g) to moles using its molar mass.
2. Use the mole ratio from the balanced equation to find the moles of NH₃ required.
3. Convert the moles of NH₃ to grams using its molar mass.
4. Use the mole ratio to find the moles of H₂O produced.
5. Convert the moles of H₂O to grams using its molar mass.
This exercise involves understanding stoichiometry, which is fundamental in chemistry for predicting the amounts of substances consumed and produced in a chemical reaction.
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