Measurements show that unknown compound x has the following composition: col1 element carbon hydrogen oxygencol2 mass % 63.2% 5.31% 31.6% write the empirical chemical formula of x. っ

The empirical formula is C8H8O3

Explanation:

Step 1: Data given

Suppose mass of the compound X is 100.00 grams

Carbon = 63.2% = 63.2 grams

Hydrogen = 5.31 % = 5.31 grams

Oxygen = 31.6 % = 31.6 grams

Molar mass of carbon = 12 g/mol

Molar mass of hydrogen = 1.01 g/mol

Molar mass of oxygen = 16 g/mol

Step 2: Calculate moles

Moles = Mass / molar mass

Moles carbon = 63.2 grams / 12 g/mol = 5.25 moles

Moles hydrogen = 5.31 grams / 1.01 g/mol = 5.25 moles

Moles oxygen : 31.6 grams / 16 g/mol ≈ 2 moles

If we multiply all by 1.5 we get the empirical formule of C8H8O3

The molar mass of the empirical formula = 152.08 g/mol

We can control this by calculating the mass %

C = ((8*12)/152.08) * 100% = 63.1 %

H = (8.08 /152.08)*100%= 5.30 %

O = ((3*16)/152.08)*100% = 31.6

8 carbon atoms forming single bonds with 18 hydrogen atoms; a triple bond exists between the third and fourth carbon atom from the right

explanation:

8 m/s because for him to get the same amount of energy as ray is putting out, bobby, who weighs half as much as ray, needs to run twice as fast.