Which of the following statements represents a key concept of Graham's Law?

Which of the following statements represents a key concept of Graham's Law?

• A. Heavier gases effuse more quickly
• B. Lighter gases diffuse faster than heavier gases
• C. The rate of diffusion is independent of molecular weight
• D. Diffusion occurs at equal rates for all gases

Answer: (B)

The key concept of Graham's Law, formulated by Thomas Graham in the 19th century, states that the rate of effusion or diffusion of a gas is inversely proportional to the square root of its molar mass. This principle implies that lighter gases, which have smaller molar masses, will diffuse or effuse faster than heavier gases, which have larger molar masses. This relationship can be mathematically expressed as the equation: \[ \frac{Rate_1}{Rate_2} = \sqrt{\frac{Molar \ mass_2}{Molar \ mass_1}} \] where Rate 1 and Rate 2 are the rates of diffusion for two different gases, and Molar mass 1 and Molar mass 2 are their respective molar masses. The implication of this relationship is that for any two gases, the lighter gas (having a lower molar mass) will diffuse more quickly than the heavier gas, highlighting the fundamental understanding of how gas particles move and behave under different conditions. In contrast, statements that suggest heavier gases effuse more quickly, that the rate of diffusion is independent of molecular weight, or that diffusion occurs at equal rates for all gases do not align with this scientific principle, as they

The key concept of Graham's Law, formulated by Thomas Graham in the 19th century, states that the rate of effusion or diffusion of a gas is inversely proportional to the square root of its molar mass. This principle implies that lighter gases, which have smaller molar masses, will diffuse or effuse faster than heavier gases, which have larger molar masses.

This relationship can be mathematically expressed as the equation:

[

\frac{Rate_1}{Rate_2} = \sqrt{\frac{Molar \ mass_2}{Molar \ mass_1}}

]

where Rate 1 and Rate 2 are the rates of diffusion for two different gases, and Molar mass 1 and Molar mass 2 are their respective molar masses. The implication of this relationship is that for any two gases, the lighter gas (having a lower molar mass) will diffuse more quickly than the heavier gas, highlighting the fundamental understanding of how gas particles move and behave under different conditions.

In contrast, statements that suggest heavier gases effuse more quickly, that the rate of diffusion is independent of molecular weight, or that diffusion occurs at equal rates for all gases do not align with this scientific principle, as they