02) and gaseo is the theoretical yield of water formed from the reaction of 9.95 g of methane and 11.5 g of oxygen gas? bus methane (CH4) reacts with gaseous oxygen gas (02) to produce gaseous carbon dioxide d your answer to 3 significant figures.
02) and gaseo is the theoretical yield of water formed from the reaction of 9.95 g of methane and 11.5 g of oxygen gas? bus methane (CH4) reacts with gaseous oxygen gas (02) to produce gaseous carbon dioxide d your answer to 3 significant figures.
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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![**Title: Calculating Theoretical Yield in Chemical Reactions**
**Introduction**
Understanding the theoretical yield of a chemical reaction is essential in fields such as chemistry and chemical engineering. Here, we present a simple example to illustrate how to calculate the theoretical yield of water produced in a chemical reaction.
---
**Problem Statement**
Gaseous methane (CH₄) reacts with gaseous oxygen gas (O₂) to produce gaseous carbon dioxide (CO₂) and gaseous water (H₂O).
**Given:**
- 9.95 grams of methane (CH₄)
- 11.5 grams of oxygen gas (O₂)
**Question:**
What is the theoretical yield of water formed from the reaction of the given amounts of methane and oxygen gas?
**Note:** Round your answer to 3 significant figures.
---
**Reaction Equation**
The balanced chemical equation for the reaction is:
\[ \text{CH}_4 + 2\text{O}_2 \rightarrow \text{CO}_2 + 2\text{H}_2\text{O} \]
---
**Steps to Calculate Theoretical Yield:**
**1. Calculate the Molar Mass:**
- Molar mass of CH₄: 12 (C) + 4 × 1 (H) = 16 g/mol
- Molar mass of O₂: 2 × 16 (O) = 32 g/mol
- Molar mass of H₂O: 2 × 1 (H) + 16 (O) = 18 g/mol
**2. Convert Grams to Moles:**
- Moles of CH₄:
\[ \frac{9.95 \text{ g}}{16 \text{ g/mol}} = 0.622 \text{ mol} \]
- Moles of O₂:
\[ \frac{11.5 \text{ g}}{32 \text{ g/mol}} = 0.359 \text{ mol} \]
**3. Determine the Limiting Reagent:**
From the balanced equation, 1 mole of CH₄ reacts with 2 moles of O₂.
- Moles of O₂ needed for 0.622 mol of CH₄:
\[ 0.622 \text{ mol CH}_4 \times 2 \text{ mol O}_2/\text{mol CH](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F88a4d88f-5648-4e4d-a49c-10af3e87c66c%2F62b6a3d0-0f75-46ce-9d4d-4579e7c03531%2F314jhb3_processed.png&w=3840&q=75)
Transcribed Image Text:**Title: Calculating Theoretical Yield in Chemical Reactions**
**Introduction**
Understanding the theoretical yield of a chemical reaction is essential in fields such as chemistry and chemical engineering. Here, we present a simple example to illustrate how to calculate the theoretical yield of water produced in a chemical reaction.
---
**Problem Statement**
Gaseous methane (CH₄) reacts with gaseous oxygen gas (O₂) to produce gaseous carbon dioxide (CO₂) and gaseous water (H₂O).
**Given:**
- 9.95 grams of methane (CH₄)
- 11.5 grams of oxygen gas (O₂)
**Question:**
What is the theoretical yield of water formed from the reaction of the given amounts of methane and oxygen gas?
**Note:** Round your answer to 3 significant figures.
---
**Reaction Equation**
The balanced chemical equation for the reaction is:
\[ \text{CH}_4 + 2\text{O}_2 \rightarrow \text{CO}_2 + 2\text{H}_2\text{O} \]
---
**Steps to Calculate Theoretical Yield:**
**1. Calculate the Molar Mass:**
- Molar mass of CH₄: 12 (C) + 4 × 1 (H) = 16 g/mol
- Molar mass of O₂: 2 × 16 (O) = 32 g/mol
- Molar mass of H₂O: 2 × 1 (H) + 16 (O) = 18 g/mol
**2. Convert Grams to Moles:**
- Moles of CH₄:
\[ \frac{9.95 \text{ g}}{16 \text{ g/mol}} = 0.622 \text{ mol} \]
- Moles of O₂:
\[ \frac{11.5 \text{ g}}{32 \text{ g/mol}} = 0.359 \text{ mol} \]
**3. Determine the Limiting Reagent:**
From the balanced equation, 1 mole of CH₄ reacts with 2 moles of O₂.
- Moles of O₂ needed for 0.622 mol of CH₄:
\[ 0.622 \text{ mol CH}_4 \times 2 \text{ mol O}_2/\text{mol CH
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