Question

If the following elements were to combine with each other, choose which demonstrate the Law of Multiple Proportion. Select all that apply.

A. 0ZX=71
B. AZ=2.5:1
C. AZ=2^21
D. DY:X=11:1

Answer 1

Option D (DY:X=11:1) demonstrates the Law of Multiple Proportions, suggesting that DY and X are different compounds composed of the same elements with masses combined in a small whole-number ratio.

Step-by-step explanation:

To determine which cases demonstrate the Law of Multiple Proportions, we need to look at the ratios provided and check if they represent different compounds made up of the same elements but in different small whole-number ratios.

According to the Law of Multiple Proportions, if elements A and B form two compounds, the different masses of A that combine with a fixed mass of B will be in the ratio of small whole numbers.

Considering the examples given:

• A. 0ZX=71 — This does not fit the format of a ratio of masses.
• B. AZ=2.5:1 — This ratio is not a small whole number and therefore does not demonstrate the Law of Multiple Proportions.
• C. AZ=2^21 — This represents a large number that does not readily indicate a ratio of masses.
• D. DY:X=11:1 — This is a ratio of small whole numbers and could represent the Law of Multiple Proportions if DY and X are different compounds with the same two elements.

Hence, option D appears to be an example that supports the Law of Multiple Proportions, suggesting that DY and X are different compounds composed of the same elements.