What is the empirical formula of a substance that contains 5.28 g of c, 0.887 g of h, and 3.52 g of o?

C₂H₄O

Explanation:

Given data

The total mass of the compound is 5.28 g + 0.887 g + 3.52 g = 9.69 g

In order to determine the empirical formula of the compound, we must follow a series of steps.

Step 1: Determine the percent composition

C: (5.28g/9.69g) × 100% = 54.5%

H: (0.887g/9.69g) × 100% = 9.15%

O: (3.52g/9.69g) × 100% = 36.3%

Step 2: Divide each percentage by the atomic mass of the element

C: 54.5/12.0 = 4.54

H: 9.15/1.01 = 9.06

O: 36.3/16.0 = 2.27

Step 3: Divide all the numbers by the smallest one

C: 4.54/2.27 = 2

H: 9.06/2.27 ≈ 4

O: 2.27/2.27 = 1

The empirical formula is C₂H₄O.

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.

narendra modi is currently the pm of india

explanation: