(a)
Interpretation:
Whether the diffusion of ammonia through an atmosphere of helium is faster or slower than through air in Example 19.9 is to be stated.
Concept introduction:
The mutual diffusion constant involves the three mean free paths, that is, between like gas particles and between the different gas particles. The mutual diffusion constant is given by,
Where,
•
•
•
•
•
•
The mutual diffusion constant does not depend on the mole fractions of the involved gases.
(b)
Interpretation:
Whether the diffusion of ammonia through an atmosphere of
Concept introduction:
The mutual diffusion constant involves the three mean free paths, that is, between like gas particles and between the different gas particles. The mutual diffusion constant is given by,
Where,
•
•
•
•
•
•
The mutual diffusion constant does not depend on the mole fractions of the involved gases.
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Physical Chemistry
- One of the chemical controversies of the nineteenth century concerned the element beryllium (Be). Berzelius originally claimed that beryllium was a trivalent element (forming Be3+ ions) and that it gave an oxide with the formula Be2O3. This resulted in a calculated atomic mass of 13.5 for beryllium. In formulating his periodic table, Mendeleev proposed that beryllium was divalent (forming Be2+ ions) and that it gave an oxide with the formula Be2O3. This assumption gives an atomic mass of 9.0. In 1894, A. Combes (Comptes Rendus 1894, p. 1221) reacted beryllium with the anion C5H7O2and measured the density of the gaseous product. Combess data for two different experiments are as follows: I II Mass 0.2022 g 0.2224 g Volume 22.6 cm3 26.0 cm3 Temperature 13C 17C Pressure 765.2 mm Hg 764.6 mm If beryllium is a divalent metal, the molecular formula of the product will be Be(C5H7O2)2; if it is trivalent, the formula will be Be(C5H7O2)3. Show how Combess data help to confirm that beryllium is a divalent metal.arrow_forwardHeavy water, D2O (molar mass = 20.03 g mol-1). can be separated from ordinary water, H2O (molar mass = 18.01), as a result of the difference in the relative rates of diffusion of the molecules in the gas phase. Calculate the relative rates of diffusion of H2O and D2O.arrow_forwardGiven that a sample of air is made up of nitrogen, oxygen, and argon in the mole fractions 0.78 N2, 0.21 O2, and 0.010 Ar, what is the density of air at standard temperature and pressure?arrow_forward
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