A sample of gas contains 0.1800 mol of CH(g) and 0.1800 mol of H,O(g) and occupies a volume of 12.3 L. The following reaction takes place: CH4(g)+ H,0(g)3H,(g) + CO(g) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant.
A sample of gas contains 0.1800 mol of CH(g) and 0.1800 mol of H,O(g) and occupies a volume of 12.3 L. The following reaction takes place: CH4(g)+ H,0(g)3H,(g) + CO(g) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant.
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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![### Chemistry Practice Problem: Gas Sample Volume Calculation
**Problem Statement:**
A sample of gas contains 0.1800 mol of \( \text{CH}_4(g) \) and 0.1800 mol of \( \text{H}_2\text{O(g)} \) and occupies a volume of 12.3 L. The following reaction takes place:
\[ \text{CH}_4(g) + \text{H}_2\text{O(g)} \rightarrow 3\text{H}_2(g) + \text{CO(g)} \]
Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant.
**Solution:**
To solve this problem, we need to follow the steps outlined below. First, identify the initial mole fractions and the stoichiometry of the reaction, then use the Ideal Gas Law as necessary.
#### Step-by-Step Solution:
1. **Reaction Stoichiometry:**
The given chemical reaction:
\[ \text{CH}_4(g) + \text{H}_2\text{O(g)} \rightarrow 3\text{H}_2(g) + \text{CO(g)} \]
indicates that one mole of \( \text{CH}_4 \) reacts with one mole of \( \text{H}_2\text{O} \) to produce three moles of \( \text{H}_2 \) and one mole of \( \text{CO} \).
2. **Initial Moles:**
Initial moles of \( \text{CH}_4 \) = 0.1800 mol
Initial moles of \( \text{H}_2\text{O} \) = 0.1800 mol
3. **Moles After Reaction:**
After the reaction, all the \( \text{CH}_4 \) and \( \text{H}_2\text{O} \) will react completely.
By stoichiometry:
- Moles of \( \text{H}_2 \) produced = \( 3 \times 0.1800 \) = 0.5400 mol
- Moles of \( \text{CO} \) produced = 0.1800 mol
4. **Total Moles After Reaction:**
Total moles of gas after the reaction = Moles](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F60358686-21d1-41ff-a93a-9ba59c7b6516%2Fb432f367-c8ce-4e55-8735-a85fcbd143f7%2Fqzjrp4r_reoriented.jpeg&w=3840&q=75)
Transcribed Image Text:### Chemistry Practice Problem: Gas Sample Volume Calculation
**Problem Statement:**
A sample of gas contains 0.1800 mol of \( \text{CH}_4(g) \) and 0.1800 mol of \( \text{H}_2\text{O(g)} \) and occupies a volume of 12.3 L. The following reaction takes place:
\[ \text{CH}_4(g) + \text{H}_2\text{O(g)} \rightarrow 3\text{H}_2(g) + \text{CO(g)} \]
Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant.
**Solution:**
To solve this problem, we need to follow the steps outlined below. First, identify the initial mole fractions and the stoichiometry of the reaction, then use the Ideal Gas Law as necessary.
#### Step-by-Step Solution:
1. **Reaction Stoichiometry:**
The given chemical reaction:
\[ \text{CH}_4(g) + \text{H}_2\text{O(g)} \rightarrow 3\text{H}_2(g) + \text{CO(g)} \]
indicates that one mole of \( \text{CH}_4 \) reacts with one mole of \( \text{H}_2\text{O} \) to produce three moles of \( \text{H}_2 \) and one mole of \( \text{CO} \).
2. **Initial Moles:**
Initial moles of \( \text{CH}_4 \) = 0.1800 mol
Initial moles of \( \text{H}_2\text{O} \) = 0.1800 mol
3. **Moles After Reaction:**
After the reaction, all the \( \text{CH}_4 \) and \( \text{H}_2\text{O} \) will react completely.
By stoichiometry:
- Moles of \( \text{H}_2 \) produced = \( 3 \times 0.1800 \) = 0.5400 mol
- Moles of \( \text{CO} \) produced = 0.1800 mol
4. **Total Moles After Reaction:**
Total moles of gas after the reaction = Moles
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