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Calculate the molecular formula for a compound whose empirical formula is [tex]\( CH_2O \)[/tex] and molar mass is [tex]\( 150.0 \, g/mol \)[/tex].

Step 1: Calculate the molar mass for the empirical formula.
What is the molar mass of [tex]\( CH_2O \)[/tex]?
( [tex]\( C = 12.01 \, amu \)[/tex], [tex]\( H = 1.01 \, amu \)[/tex], [tex]\( O = 16.00 \, amu \)[/tex] )
[tex]\[ \boxed{?} \, g/mol \, CH_2O \][/tex]



Answer :

GinnyAnswer
To calculate the molar mass of the empirical formula [tex]\( CH_2O \)[/tex], we need to sum up the contributions of each element based on their respective atomic masses and the number of each atom in the empirical formula.

1. The molar mass of Carbon (C) is [tex]\( 12.01 \, \text{amu} \)[/tex].
2. The molar mass of Hydrogen (H) is [tex]\( 1.01 \, \text{amu} \)[/tex].
3. The molar mass of Oxygen (O) is [tex]\( 16.00 \, \text{amu} \)[/tex].

The empirical formula [tex]\( CH_2O \)[/tex] consists of:
- 1 atom of Carbon
- 2 atoms of Hydrogen
- 1 atom of Oxygen

We calculate the molar mass of [tex]\( CH_2O \)[/tex] by summing up the contributions:

[tex]\[ \text{Molar mass of } CH_2O = (1 \times 12.01) + (2 \times 1.01) + (1 \times 16.00) \][/tex]

Simplifying the calculations:

[tex]\[ \text{Molar mass of } CH_2O = 12.01 + 2.02 + 16.00 \][/tex]

[tex]\[ \text{Molar mass of } CH_2O = 30.03 \, \text{g/mol} \][/tex]

Therefore, the molar mass of [tex]\( CH_2O \)[/tex] is [tex]\( 30.03 \, \text{g/mol} \)[/tex].

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