Understanding Graham's Law
Graham's Law of Diffusion states that the rate of diffusion of a gas is inversely proportional to the square root of its molar mass.
* Higher Molar Mass = Slower Diffusion
* Lower Molar Mass = Faster Diffusion
Applying Graham's Law
1. Density and Molar Mass: Since density is directly related to molar mass (assuming constant pressure and temperature), we can use the density ratio to compare their diffusion rates.
2. Calculating the Ratio:
* Gas A is 16 times denser than Gas B. This means Gas A has 16 times the molar mass of Gas B.
* Let's say the molar mass of Gas B is 'M'. Then the molar mass of Gas A is '16M'.
3. Diffusion Rate Ratio:
* Rate of diffusion of Gas A / Rate of diffusion of Gas B = √(Molar mass of B) / √(Molar mass of A)
* Rate of diffusion of Gas A / Rate of diffusion of Gas B = √(M) / √(16M) = 1/4
Conclusion
* Gas B diffuses four times faster than Gas A. This is because it has a significantly lower molar mass (and therefore a lower density).
