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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)

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ardni313

The empirical formula : CH₂O  

The molecular formula : C₈H₁₆O₈

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

Further explanation  

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

  • Determine the mass ratio of the constituent elements of the compound.  
  • Determine the mole ratio by dividing the elemental mass with the relative atomic mass obtained by the empirical formula  
  • Determine molecular formulas by looking for values of n  

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

Learn more  

the molar mass of a substance  

brainly.com/question/837939  

Determine the empirical and molecular formulas  

brainly.com/question/9255428  

Determine the molecular formula of the compound  

brainly.com/question/11558543  

Keywords: empirical formula, molecular formula, mass, mole  

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dsdrajlin

There is a missing part. I think the complete question is:

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).

The compound with a composition of 40.0 % C, 6.70% H, and 53.3% O by mass and a molecular mass of 240 amu, has a molecular formula of C₈H₁₆O₈. The subscripts are 8,16,8.

First, we will determine the empirical formula of the compound. The first step is to divide the percentage by mass of each element by its atomic mass.

[tex]C: 40.0/12.01 = 3.33\\H: 6.70/1.01 = 6.63\\O: 53.3/16.00 = 3.33[/tex]

Then, we divide all the numbers by the smallest one, i.e. 3.33.

[tex]C: 3.33/3.33 = 1\\H: 6.63/3.33 \approx 2\\O: 3.33/3.33 = 1[/tex]

The empirical formula is CH₂O. The molar mass of the empirical formula is:

[tex]M(CH_2O) = MC + 2MH + MO = 12.01 g/mol + 2(1.01 g/mol) + 16.00 g/mol = 30.03 g/mol[/tex]

Next, we calculate "n", which is the quotient between the molar mass of the molecular formula (240 g/mol) and the molar mass of the empirical formula (30.03 g/mol).

[tex]n = \frac{240g/mol}{30.03 g/mol} \approx 8[/tex]

The molecular formula is "n"  times (8 times) the empirical formula.

[tex]CH_2O \times 8 = C_8H_{16}O_8[/tex]

The compound with a composition of 40.0 % C, 6.70% H, and 53.3% O by mass and a molecular mass of 240 amu, has a molecular formula of C₈H₁₆O₈. The subscripts are 8,16,8.

You can learn more about empirical and molecular formula here: https://brainly.com/question/14425592

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