Question

(i) a certain pure compound containing element e is analyzed. the elemental composition of the compound is shown in the following table. determine the empirical formula of the compound using the information in the table.

element	moles present in the compound
s	0.0338
o	0.102

Explanation:

Step1: Find the smallest mole value

First, identify the moles of each element: E has \( 0.0676 \) mol, S has \( 0.0338 \) mol, O has \( 0.102 \) mol. The smallest value is \( 0.0338 \) (moles of S).

Step2: Divide each mole by the smallest

• For E: \( \frac{0.0676}{0.0338} = 2 \)
• For S: \( \frac{0.0338}{0.0338} = 1 \)
• For O: \( \frac{0.102}{0.0338} \approx 3 \) (since \( 0.0338\times3 = 0.1014 \approx 0.102 \))

Step3: Determine the empirical formula

Using the ratios from Step 2, the empirical formula is \( \text{E}_2\text{SO}_3 \) (or check if the ratios are whole numbers: E:2, S:1, O:3, all whole numbers).

Answer:

The empirical formula of the compound is \( \boldsymbol{\text{E}_2\text{SO}_3} \) (or depending on the actual element E, but the ratio gives E₂SO₃).