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times that of Br, (g) under the same conditions. Ne(g) effuses at a rate that is . ratese ratepr, =

times that of Br, (g) under the same conditions. Ne(g) effuses at a rate that is . ratese ratepr, =

Chemistry
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 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.
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.
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Here, we have to find the ratio of the rate of effusion of Ne (g) to the rate of effusion of Br2 (g).

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