Question

2.48925 C: 3.9901 H: 1.000 O The ratio does not give whole numbers, so we have to use a multiplier. What can we multiply each element by in order to have them all reach the smallest whole number? multiply by [?] Hint: The multiplier should be a whole number.​

Answer 1

To convert the atomic ratios of C: 2.48925, H: 3.9901, O: 1.000 to whole numbers, we should multiply each by 3. This yields integer values and suggests an empirical formula of C3H4O3, with a simplified ratio of C:H:O as 3:4:3.

Step-by-step explanation:

The student's question relates to finding the multiplier that would convert non-integer atomic ratios to the smallest whole numbers in a chemical formula. When trying to establish the empirical formula of a compound, it's essential to have integer ratios. Given the atomic ratios for carbon (C), hydrogen (H), and oxygen (O), as 2.48925:3.9901:1.000, the goal is to convert these relative atomic amounts into a simple whole-number ratio. The student has noted that the ratios do not yield whole numbers and thus require a multiplier.

To normalize the amount of hydrogen to an integer, we should look at the decimal component of the ratio, which suggests the number may be approximately one and one-third (1.333). Therefore, to convert these amounts to integers, multiplying by 3 is appropriate. After multiplying, we get whole numbers for each element, resulting in a simple whole-number ratio of C:H:O as 3:4:3, which suggests an empirical formula of C3H4O3.

Remember, the empirical formula represents the simplest ratio of the elements in a compound and is derived by identifying the smallest whole-number multiples for the given molar amounts.