Determine the empirical formula for compounds that have the following analyses: a. 66.0% barium and 34.0% chlorine b. 80.38% bismuth, 18.46% oxygen, and 1.16% hydrogen.

a)

b)  

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.

a) Mass of Ba= 66.06 g

Mass of Cl = 34.0 g

Step 1 : convert given masses into moles.

Moles of Ba =

Moles of Cl = \frac{\text{ given mass of Cl}}{\text{ molar mass of Cl}}= \frac{34g}{35.5g/mole}=0.96moles[/tex]

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

For Ba =

For O =

The ratio of Ba: Cl= 1:2

Hence the empirical formula is

b) Mass of Bi= 80.38 g

Mass of O= 18.46 g

Mass of H = 1.16 g

Step 1 : convert given masses into moles.

Moles of Bi =

Moles of O=

Moles of H=

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

For Bi=

For O =

For H=

The ratio of Bi: O: H= 1:3: 3

Hence the empirical formula is

the answer is 303.15 or 303