Question

A compound contains 64 g of o and 8 g of h. what is the empirical formula for this compound?

Answer 1

The empirical formula is obtained by calculating the mole ratios of the atoms in the elements.
The number of moles =mass/ R.A.M
For hydrogen, no. of moles=8/1=8
For oxygen, no. Of moles=64/16=4
The tabular solution is attached.

Answer 2

Answer:

The compound is the H2O

Explanation:

In order to calculate the empirical formula of any compound, we should only follow three steps:

1. Calculate the moles of each element of the compound using percentage or mass.

2. Calculate the ratio of each mole.

3. Write the empirical formula

With these 3 steps, we can easily calculate the empirical formula of any compound.

We have masses here, so, let's do this in the 3 steps:

1. moles of each element

To do this, we need the molecular mass of each element. In the case of Hydrogen is 1 g/mol and the case for Oxygen is 16 g/mol so:

H: 8/1 = 8 moles

O: 64/16 = 4 moles

2. ratio of moles of each element

To do this, we should divide each moles between the lowest moles obtained in step 1. When we do this, the final result will give the number of atoms of each element in the formula. So doing this:

H: 8/4 = 2

O: 4/4 = 1

This means that we have 2 atoms of H, and 1 of oxygen.

3. Write the empirical formula

Now that we have the number of atoms, we should only write the elements and the atoms obtained in step 2.

Empirical Formula: H2O