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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Question
Question 2
![### Gas Effusion Rates
**Problem Statement:**
Ne(g) effuses at a rate that is ______ times that of Br₂(g) under the same conditions.
**Equation:**
\[ \text{rate}_{\text{Ne}} \]
\[ \text{rate}_{\text{Br}_2} \]
**Explanation:**
This problem involves comparing the effusion rates of different gases, which is often calculated using Graham's law of effusion. The law states that the rate of effusion of a gas is inversely proportional to the square root of its molar mass. Therefore, the ratio of the effusion rates of two gases can be determined by the following formula:
\[ \frac{\text{rate}_{\text{Ne}}}{\text{rate}_{\text{Br}_2}} = \sqrt{\frac{M_{\text{Br}_2}}{M_{\text{Ne}}}} \]
Here, \( M_{\text{Ne}} \) and \( M_{\text{Br}_2} \) represent the molar masses of neon and bromine gas, respectively. This relationship means that a lighter gas will effuse faster than a heavier gas under the same temperature and pressure conditions.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe4db1e84-75df-498d-9686-5cabfd0e0c2f%2F014ff6de-a5c6-4179-a290-34d5a23cd7c5%2F7y18hxr_processed.png&w=3840&q=75)
Transcribed Image Text:### Gas Effusion Rates
**Problem Statement:**
Ne(g) effuses at a rate that is ______ times that of Br₂(g) under the same conditions.
**Equation:**
\[ \text{rate}_{\text{Ne}} \]
\[ \text{rate}_{\text{Br}_2} \]
**Explanation:**
This problem involves comparing the effusion rates of different gases, which is often calculated using Graham's law of effusion. The law states that the rate of effusion of a gas is inversely proportional to the square root of its molar mass. Therefore, the ratio of the effusion rates of two gases can be determined by the following formula:
\[ \frac{\text{rate}_{\text{Ne}}}{\text{rate}_{\text{Br}_2}} = \sqrt{\frac{M_{\text{Br}_2}}{M_{\text{Ne}}}} \]
Here, \( M_{\text{Ne}} \) and \( M_{\text{Br}_2} \) represent the molar masses of neon and bromine gas, respectively. This relationship means that a lighter gas will effuse faster than a heavier gas under the same temperature and pressure conditions.
Expert Solution
Step 1
Here, we have to find the ratio of the rate of effusion of Ne (g) to the rate of effusion of Br2 (g).
Step by step
Solved in 2 steps with 1 images
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