What is the empirical formula for a compound that contains 10.89% magnesium 31.77% chloride and 57.34% oxygen

The empirical formula for a compound that contains 10.89% magnesium 31.77% chloride and 57.34% oxygen is

In the case when percentages are provided so we are taking total mass is 100 grams. So, the mass of each element should be equivalent to the percentage given.

Mass of Mg = 10.89 g

Mass of Cl = 31.77 g

Mass of O = 57.34 g

Now convert given masses into moles

So,

Moles of Mg= = 0.45 moles

Moles of Cl = = 0.89 moles

Moles of O = = 3.58 moles

Now the mole ratio is

For Mg = = 1

For Cl = = 2

For O = = 8

learn more about oxygen here: link

Explanation:

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 Mg = 10.89 g

Mass of Cl = 31.77 g

Mass of O = 57.34 g

Step 1 : convert given masses into moles.

Moles of Mg=

Moles of Cl =

Moles of O =

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

For Mg =

For Cl =

For O=

The ratio of Mg :Cl : O= 1 : 2 : 8

Hence the empirical formula is

the density(ratio between mass and volume as m/v) decreases from top to bottom in periodic table group as the size increases and nuclear charge decreases. but in periods density increases from left to right as atom size decreases and nuclear charge increases.

1 is the answer to this problem