SDSU Chemistry Placement Test 2025 – Complete Practice for Exam Preparation

Question: 1 / 400

According to Graham's Law, what is the relationship between gas diffusion rates and molar masses?

r1/r2 = MM2/MM1

r1/r2 = MM1/MM2

Graham's Law states that the rates of diffusion of two gases are inversely proportional to the square roots of their molar masses. This means that lighter gases diffuse more quickly than heavier gases. The correct mathematical expression of this relationship is given by the formula:

\[

\frac{r_1}{r_2} = \sqrt{\frac{MM_2}{MM_1}}

\]

To make the relationship more intuitive, we can rearrange this formula by squaring both sides, which gives us:

\[

\frac{r_1^2}{r_2^2} = \frac{MM_2}{MM_1}

\]

From this, it becomes clear that the ratio of their rates of diffusion (r1/r2) can be expressed in terms of their molar masses. Thus, when taking the square roots and rearranging, the correct relationship can be derived as:

\[

\frac{r_1}{r_2} = \sqrt{\frac{MM_2}{MM_1}} \text{ or in a more familiar form } \frac{r_1}{r_2} = \frac{MM_1}{MM_2}

\]

This correctly reflects

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r1 + r2 = MM1 + MM2

r1 - r2 = MM1 - MM2

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