The molecular formula mass of this compound is 240 amu . what are the subscripts in the actual molecular formula? enter the subscripts for c, h, and o, respectively, separated by commas (e. g., 5,6,7)

The empirical formula : CH₂O  

The molecular formula : C₈H₁₆O₈

the subscripts for C, H, and O : 8,16,8  

The empirical formula is the smallest comparison of atoms of compound forming elements.  

A molecular formula is a formula that shows the number of atomic elements that make up a compound.  

(empirical formula) n = molecular formula  

The principle of determining empirical formula and molecular formula

Percentage of elements A and B in AxBy compounds:  

% A in AₓBy = (x x Ar A / Mr AₓBy) x% AₓBy  

% B in AₓBy = (y x Ar B / Mr AₓBy) x% AₓBy  

It is known about the% mass of each element  

The complete question must be :

A Compound Is 40.0 % C, 6.70% H, And 53.3% O By Mass. Assume That We Have A 100g Sample Of This Compound. The Molecular Formula Mass Of This Compound Is 240 Amu. what are the subscripts in the actual molecular formula? enter the subscripts for c, h, and o, respectively, separated by commas (e.g., 5,6,7)

To find the empirical formula, we look for its mole ratio (% mass/ its relative atomic mass)  

C = 40 / 12 = 3.3

H = 6.70/ 1 = 6.70

O = 53.3 / 16 = 3.3

To simplify the comparison as an integer, we divide by the mole ratio of the smallest element  

C = 3.3/3.3= 1

H = 6.7 /3.3 = 2

O = 3.3/3.3 = 1  

So the empirical formula:  

CH₂O  

We look for the molecular formula to get the number of atoms making up the compound  

(CH₂O) n = molecular formula  

(1.12 + 2.1 + 16) n = 240

(30) n = 240

n = 8

So molecular formula = C₈H₁₆O₈

the molar mass of a substance  

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Determine the empirical and molecular formulas  

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Determine the molecular formula of the compound  

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Keywords: empirical formula, molecular formula, mass, mole  

2b2t

explanation:

2b2t