What is the empirical formula of a compound composed of 3.25% hydrogen ( H ), 19.36% carbon ( C ), and 77.39% oxygen ( O ) by mass? Insert subscripts as needed.

Answer : The empirical of the compound is,

Solution : Given,

If percentage are given then we are taking total mass is 100 grams.

So, the mass of each element is equal to the percentage given.

Mass of C = 19.36 g

Mass of H = 3.25 g

Mass of O = 77.39 g

Molar mass of C = 12 g/mole

Molar mass of H = 1 g/mole

Molar mass of O = 16 g/mole

Step 1 : convert given masses into moles.

Moles of C =

Moles of H =

Moles of O =

Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.

For C =

For H =

For o =

The ratio of C : H : O = 1 : 2 : 3

The mole ratio of the element is represented by subscripts in empirical formula.

The Empirical formula =

Therefore, the empirical of the compound is,

fe 55.85 g/mol and h2o 18.02 g/mol.

c. electrical charges of ionic bonds.