GIVING BRAINLISTED PLEASE ONLY ANSWER IF YOU KNOW THE ANSWER

Determine the empirical formula of a compound containing 48.38 grams of carbon, 6.74 grams of hydrogen, and 53.5 grams of oxygen.

In an experiment, the molar mass of the compound was determined to be 180.15 g/mol. What is the molecular formula of the compound?

For both questions, show your work or explain how you determined the formulas by giving specific values used in calculations.

#Divide given mass with their molar masses.

C=48.38÷12.01= 4.03mols

H= 6.74÷1.0079= 6.69mols

O= 53.5÷16.00= 3.34mols

#Divide the moles with the lowest mole.

C = 4.03÷3.34 = 1.21

H = 6.69÷3.34 = 2.00

O = 3.34÷3.34 = 1

∴Emperical Formula = CH₂O

#Molar mass of CH₂O = 12.01 + (1.0079 x 2) + 16.00 = 30.02 g/mol

#Divide both moler masses: 180.15g/mol÷30.02g/mol = 6

#Multiply the answer with the Emperical formula to get the Molecular formula: 6 x (CH₂O) = C₆H₁₂O₆

Explanation:

  the   balanced   equation   for   reaction of   ca metal   with   o2 to   produce   cao   is as below

2 ca+ o2→ 2 cao2

  explanation

the reaction is   balanced     since the   number of atoms   in reactant side is   equal to   number of atoms   in   product side.   for   example   they   are 2   atom of   ca in   reactant   side   and   2   atoms of ca   in   the product side.

  the   process   is a   meet the   requirement   of   redox   reaction because :     calcium   is   oxidized   from   oxidation state 0   to 2+   while   oxygen   is reduced from   oxidation   state   0   to 2-

personal, she chose to do it.