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Medium
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A vessel contains two nonreactive gases : neon (monatomic) and oxygen (diatomic). The ratio of their partial pressures is 3:2. Estimate the ratio of (i) number of molecules and (ii) mass density of neon and oxygen in the vessel. Atomic mass of , molecular mass of .
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Partial pressure of a gas in a mixture is the pressure it would have for the same volume and temperature if it alone occupied the vessel. (The total pressure of a mixture of non-reactive gases is the sum of partial pressures due to its constituent gases.) Each gas (assumed ideal) obeys the gas law. Since and are common to the two gases, we have and , i.e. . Here 1 and 2 refer to neon and oxygen respectively. Since (3/2) (given), .
(i) By definition and where and are the number of molecules of 1 and 2 , and is the Avogadro's number. Therefore, .
(ii) We can also write and where and are the masses of 1 and 2 ; and and are their molecular masses. (Both and ; as well as and should be expressed in the same units). If and are the mass densities of 1 and 2 respectively, we have
(i) By definition and where and are the number of molecules of 1 and 2 , and is the Avogadro's number. Therefore, .
(ii) We can also write and where and are the masses of 1 and 2 ; and and are their molecular masses. (Both and ; as well as and should be expressed in the same units). If and are the mass densities of 1 and 2 respectively, we have
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Question Text | A vessel contains two nonreactive gases : neon (monatomic) and oxygen (diatomic). The ratio of their partial pressures is 3:2. Estimate the ratio of (i) number of molecules and (ii) mass density of neon and oxygen in the vessel. Atomic mass of , molecular mass of . |
Updated On | Apr 2, 2023 |
Topic | Thermodynamics |
Subject | Physics |
Class | Class 11 |
Answer Type | Text solution:1 Video solution: 1 |
Upvotes | 182 |
Avg. Video Duration | 4 min |