A compound is found to contain 9.224 % boron and 90.74 % chlorine by mass. To answer the question, enter the elements in the order presented above. QUESTION 1: The empirical formula for this compound is . QUESTION 2: The molar mass for this compound is 117.2 g/mol. The molecular formula for this compound is .

Empirical formula of a compound means that it provides simplest ratio of whole number.

Explanation:

QUESTION-1

Given,

Mass of boron and chlorine is 9.224% and 90.74%

Then, Boron- 9.224×=0.85 mol   (Mass value of boron=10.811)

      Chlorine- 90.74×=2.559 mol.(Mass value of chlorine=35.453)

By dividing the mole value with smallest number, then we will get-

Boron-=1

Chlorine-=3

The empirical formula of the compound is -BCl₃

QUESTION-2

BCl₃⇄B+ 3.Cl  (Putting the actual mass number of boron and chlorine we will get-)

           1×(10.811)+ 3×(35.453)=117.17g/mol

Molecular formula=

                               = ≈1

  The molecular formula is same with the empirical formula.

idk

explanation:

dasdad

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.