Respuesta :
Answer: [tex]Mg_{1}Cl_{2}O_{8}[/tex]
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=[tex]\frac {\text{ given mass of Mg}}{\text{ molar mass of Mg}}= \frac {10.89g}{24g/mole}=0.45moles[/tex]
Moles of Cl = [tex]\frac {\text{ given mass of Cl}}{\text{ molar mass of Cl}}= \frac {31.77g}{35.5g/mole}=0.89moles[/tex]
Moles of O =[tex]\frac {\text{ given mass of O}}{\text{ molar mass of O}}=\frac {57.34g}{16g/mole}=3.58moles[/tex]
Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.
For Mg = [tex]\frac {0.45}{0.45}=1[/tex]
For Cl = [tex]\frac {0.89}{0.45}=2[/tex]
For O= [tex]\frac {3.58}{0.45}=8[/tex]
The ratio of Mg :Cl : O= 1 : 2 : 8
Hence the empirical formula is [tex]Mg_{1}Cl_{2}O_{8}[/tex]
The empirical formula for a compound that contains 10.89% magnesium 31.77% chloride and 57.34% oxygen is [tex]Mg_1Cl_2O_8[/tex]
Empirical formula:
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=[tex]10.89 \div 24[/tex] = 0.45 moles
Moles of Cl = [tex]31.77 \div 35.5[/tex] = 0.89 moles
Moles of O = [tex]57.34 \div 16[/tex] = 3.58 moles
Now the mole ratio is
For Mg = [tex]0.45 \div 0.45[/tex] = 1
For Cl = [tex]0.89 \div 0.45[/tex] = 2
For O = [tex]3.58 \div 0.45[/tex] = 8
learn more about oxygen here: https://brainly.com/question/20856989
