Question

You have a 50.00 gram sample of a compound whose molecular weight is 180.156. On decomposition, the weights of
the component elements are 20.00 grams of carbon, 3.36 grams of hydrogen, and 26.64 grams of orygen,
The molecular formula for the compound is c o

Answer 1

Answer:

C6H12O6

Explanation:

Had the same question and it said it was the right answer :)

Answer 2

Answer:

C6 H12 O6

Explanation:

Find the percent composition of the elements:

20.00 / 50.00 × 100% = 40.00% carbon

3.36 / 50.00 × 100% = 6.72% hydrogen

26.64 / 50.00 × 100% = 53.28% oxygen

From the periodic table, the molar masses of carbon, hydrogen, and oxygen are 12.011 g/mol, 1.008 g/mol and 15.999 g/mol, respectively.

Next, divide the element’s percentage-based mass by its molar mass to get a ratio of moles:

40.00 / 12.011 = 3.33 moles of carbon

6.72 / 1.008= 6.67 moles of hydrogen

53.28 / 15.999 = 3.33 moles of oxygen

Divide each result by the lowest number of moles to obtain a 1 : x ratio:

3.33 / 3.33 = 1 mole of carbon

6.67 / 3.33 ≈ 2 moles of hydrogen

3.33 / 3.33= 1 mole of oxygen

Since each result is a whole number, the empirical formula is CH2O.

The empirical formula weight is

(1 × 12.011 grams/mole) + (2 × 1.008 grams/mole) + (1 × 15.999 grams/mole) = 30.026 grams/mole.

To find the molecular formula, divide the molecular weight by the empirical weight:

180.156 / 30.026 = 6.

So, the molecular formula has 6 times the number of each element as the empirical formula.

The molecular formula is C6 H12 O6 :)