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

The empirical formula of X is  C8H8O3

Explanation:

Step 1: Data given

Suppose the mass = 100.00 gram

A compound contains:

⇒ 63.2 % carbon = 63.2 grams

⇒ 5.31 % hydrogen = 5.31 grams

⇒ 31.6 % oxygen = 31.6 grams

Molar mass of carbon = 12.01 g/mol

Molar mass of hydrogen = 1.01 g/mol

Molar mass of oxygen = 16 g/mol

Step 2: Calculate number of moles

(63.2 g C) / (12.01 g/mol) =  5.26 mol C arbon

(5.32 g H) / (1.01 g/mol) = 5.27 mol H ydrogen

(31.6 g O) / (16.00 g/mol) = 1.975 mol O

Step 3: Calculate mol ratio

Divide by the smallest number of moles:

C: 5.26/ 1.975 = 2.66

H: 5.27 /1.975 = 2.67

O: 1.975/1.975 = 1

To achieve integer coefficients, we multiply by 3:

The empirical formula of X is  C8H8O3

a) the particles of the chair are strongly held together.

water and alcohols have similar properties because water molecules contain hydroxyl groups that can form hydrogen bonds with other water molecules and with alcohol molecules, and likewise alcohol molecules can form hydrogen bonds with other alcohol molecules as well as with water.