2. What is the empirical formula of a compound composed d of 3.26 g of arsenic and I .04 g of oxygen?

## Step 1<br />The empirical formula compound is the simplest whole number ratio of atoms of each element in the compound. To find the empirical formula, we first need to convert the given masses of each element to moles. This is done by dividing the mass of each element by its atomic mass.<br /><br />### **Moles = \(\frac{Mass}{Atomic\,Mass}\)**<br /><br />## Step 2<br />The atomic mass of arsenic (As) is approximately 74.92 g/mol, and the atomic mass of oxygen (O) is approximately 16.00 g/mol.<br /><br />## Step 3<br />Calculate the moles of arsenic and oxygen:<br /><br />### **Moles of As = \(\frac{3.26g}{74.92g/mol} = 0.0433 mol\)**<br />### **Moles of O = \(\frac{1.04g}{16.00g/mol} = 0.065 mol\)**<br /><br />## Step 4<br />The ratio of moles of arsenic to oxygen is then calculated.<br /><br />### **Ratio = \(\frac{Moles\,of\,As}{Moles\,of\,O} = \frac{0.0433}{0.065} = 0.66\)**<br /><br />## Step 5<br />The ratio is approximately 1:1, which means the empirical formula of the compound is AsO.