Explanation
Given data,
6.4 g of SO2 at 0oC and 0.99 atm pressure occupies a volume of 2.241L.
If we observe the data all the terms like T, p, V are approximately at standard conditions. Hence we can predict that the gas is ideal.
From ideal gas equation
PV = nRT
V ∝1/P
V ∝ T
P ∝ T
As the volume increases , temperature also increases and pressure decreases.
As the temperature increases, pressure also increases.
Hence the order is , P1 > P3 > P2 .
According to Graham’s law of diffusion, Rate of diffusion depends upon the molecular masses of the gases. Therefore more the rate of diffusion, lesser will be the molecular mass and vise versa.
∴The order od molecular weight of given gases of A, B and C are 2, 4, 28 respectively. Hence the order of rate of diffusion of gases is A > B > C.
From an ideal equation,
pV = nRT
where, R is known as universal gas constant or molar gas constant.
Values of R = 0.0821 L atm K–1 mol–1
= 8.314 × 107 ergs K–1 mol–1
= 8.314 J K–1 mol–1
= 1.987 = 2 cal K–1 mol–1
Hence, R is considered as a universal gas constant. It will not depend on pressure and nature of gas but depend only on the units of measurements.
According to Graham’s lae, Rate of diffusion depends upon the molecular masses of gases. Here the NH3 diffuses more quickly than the HCl. This is because the size of molecule of NH3 is smaller than that of a molecule of HCl. The molecule weight of ammonia is 17, while that of hydrogenchloride(HCl) is 36.5.
Therefore a gas effuses or diffuses at a greater rate when the molecular mass is smaller, which is another way of saying, the particles can more quickly through the air in the tube. Therefore, NH3 molecules are moving more quickly down the tube than the HCl molecules and they meey more towards the HCl end. When they meet, the reaction occurs between the two and the ring forms where the reaction occurs. Therefore, the ring is close to HCl side.
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