Question

What is the molecular formula of the molecule that has an empirical formula of CH2O and a molar mass of 120.12 g/mol

Answer 1

Answer:

C4H8O4

Explanation:

Let (CH20)x

C=1*12.01=12.01     (12.01, 1.01, 16.00 Avg mass of elements)

H=2*1.01=2.01

O=1*16.00=16.00

12.01 + 2.01 + 16.00 = 30.03

120.12/30,03=4

==> (CH2O)4 = C4H8O4

Answer 2

The molecular formula of the molecule that has an empirical formula of $CH_2O$ is equal to $C_4H_8O_4$.

Given the following data:

• Empirical formula = $CH_2O$

• Molar mass = 120.12 g/mol.

Scientific data:

• Molar mass of oxygen = 16 g/mol.

• Molar mass of hydrogen = 1 g/mol.

• Molar mass of carbon = 12 g/mol.

To determine the molecular formula of the molecule that has an empirical formula of $CH_2O$:

First of all, we would find the molar mass of $CH_2O$:

$CH_2O =12 +(1\times2)+16\\\\CH_2O =30\;g/mol$

For molecular formula:

$(CH_2O)n = 120.12\\\\30n = 120.12\\\\n=\frac{120.12}{30}$

n = 4.0

$(CH_2O)_4 = C_4H_8O_4$

Read more: https://brainly.com/question/21280037