Chemistry College

When 11.3 g 11.3 g of an organic compound known to be 70.58% C 70.58 % C , 5.9% H 5.9 % H , and 23.50% O 23.50 % O by mass is dissolved in 622.7 g 622.7 g of cyclohexane, the freezing point is 3.82 ∘C 3.82 ⁢ ∘ C . The normal freezing point of cyclohexane is 6.59 ∘C 6.59 ⁢ ∘ C . What is the molecular formula for the organic compound? Assume that the organic compound is a molecular solid and does not ionize in water. f f values for various solvents are given in the colligative constants table.

When 11.3 G 11.3 G Of An Organic Compound Known To Be 70.58% C 70.58 % C , 5.9% H 5.9 % H , And 23.50%

Answers

Answer 1

The molecular formula for the organic compound is C4H4O.

To determine the molecular formula of the organic compound, we need to calculate the number of moles of carbon (C), hydrogen (H), and oxygen (O) in the compound and find the simplest whole number ratio between them.

Given:

Mass of the organic compound = 11.3 g

Percentage composition:

Carbon (C) = 70.58%

Hydrogen (H) = 5.9%

Oxygen (O) = 23.50%

First, we calculate the mass of each element in the organic compound:

Mass of C = 70.58% of 11.3 g = 7.986 g

Mass of H = 5.9% of 11.3 g = 0.667 g

Mass of O = 23.50% of 11.3 g = 2.655 g

Next, we convert the masses of each element to moles using their respective molar masses:

Molar mass of C = 12.01 g/mol

Molar mass of H = 1.008 g/mol

Molar mass of O = 16.00 g/mol

Moles of C = 7.986 g / 12.01 g/mol ≈ 0.665 mol

Moles of H = 0.667 g / 1.008 g/mol ≈ 0.661 mol

Moles of O = 2.655 g / 16.00 g/mol ≈ 0.166 mol

Now, we divide the moles of each element by the smallest number of moles to find the simplest whole number ratio:

C: 0.665 mol / 0.166 mol ≈ 4

H: 0.661 mol / 0.166 mol ≈ 4

O: 0.166 mol / 0.166 mol = 1

Therefore, the empirical formula of the organic compound is C4H4O.

To find the molecular formula, we need to determine the molecular weight of the compound. Given that the molecular weight of the compound is 11.3 g, which is equal to the empirical formula weight (C4H4O), we can conclude that the molecular formula is the same as the empirical formula.

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Answer:

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