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...
Related questions
Question
![**Effusion Rate Comparison: Ne(g) vs. Cl₂(g)**
Under the same conditions, Ne(g) effuses at a rate that is _____ times that of Cl₂(g).
**Equation:**
\[
\frac{\text{rate}_{\text{Ne}}}{\text{rate}_{\text{Cl}_2}} = \, \rule{4cm}{0.15mm}
\]
The equation provided is used to compare the rates of effusion of neon gas (Ne) and chlorine gas (Cl₂). To determine the missing value, Graham's Law of Effusion can be applied, which states that the rate of effusion of a gas is inversely proportional to the square root of its molar mass. This means that lighter gases effuse faster than heavier gases.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa563c0cc-a924-4c37-9f6b-c4caff62891a%2Faecd711f-1806-4c76-87d2-999fcafa0eee%2Fysp1ye_processed.png&w=3840&q=75)
Transcribed Image Text:**Effusion Rate Comparison: Ne(g) vs. Cl₂(g)**
Under the same conditions, Ne(g) effuses at a rate that is _____ times that of Cl₂(g).
**Equation:**
\[
\frac{\text{rate}_{\text{Ne}}}{\text{rate}_{\text{Cl}_2}} = \, \rule{4cm}{0.15mm}
\]
The equation provided is used to compare the rates of effusion of neon gas (Ne) and chlorine gas (Cl₂). To determine the missing value, Graham's Law of Effusion can be applied, which states that the rate of effusion of a gas is inversely proportional to the square root of its molar mass. This means that lighter gases effuse faster than heavier gases.
Expert Solution
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Step 1
According to Graham's law of effusion, the effusion rate is directly proportional to the root mean square velocity(VRMS) of gas molecule.
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