kimberlylove387
30.06.2020 •
Chemistry
6.
A given volume of nitrogen gas required 68.3 seconds to diffuse through a tiny hole
in chamber. Under the same conditions, another unknown gas requires 85.6 seconds for
the same volume to diffuse. What is the molecular mass of this gas?
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Ответ:
Molar mass of the unknown gas is 8.96g/mol
Explanation:
Hello,
According to Graham's law of diffusion, its states that the rate of diffusion of a gas is inversely proportional to the square root of its molecular mass
R = k (1/√(M))
R = rate of diffusion
M = molecular mass
R₁ / R₂ = √(M₂ / M₁)
R₁ = nitrogen = 68.3s
R₂ = unknown gas = 85.6s
M₂ = molecular mass of the unknown gas
M₁ = molecular mass of nitrogen = 14g/mol
68.3 / 85.6 = (√M₂ / 14)
0.8 = (√M₂ / 14)
Take square of both sides
0.8² = M₂ / 14
M₂ = 14 × 0.64
M₂ = 8.96g/mol
The molar mass of the unknown gas is 8.96g/mol
Ответ:
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Explanation: euy 67f chrurfb