Here's how we can approach this problem once we know the second element:
1. Assume 100 grams of the compound: This makes the percentages directly translate to grams.
2. Convert grams to moles: Divide the mass of each element by its molar mass (found on the periodic table).
3. Find the simplest whole-number ratio: Divide the number of moles of each element by the smallest number of moles calculated. This will give you the subscripts for the empirical formula.
Example:
Let's say the compound is 78.14% boron and 21.86% hydrogen.
1. Grams: 78.14 g B and 21.86 g H
2. Moles:
* B: 78.14 g / 10.81 g/mol = 7.23 mol B
* H: 21.86 g / 1.01 g/mol = 21.64 mol H
3. Ratio:
* B: 7.23 mol / 7.23 mol = 1
* H: 21.64 mol / 7.23 mol = 3
Therefore, the empirical formula of the compound is BH₃.
Please provide the second element in the compound, and I can help you determine the empirical formula!
