Question

What is the molecular formula for a compound that is 40% Carbon, 6.7%

Hydrogen, and 53.3% Oxygen with a molar mass of 90 amu?
Your answer

Answer 1

C1H201 or COH2

Step-by-step explanation:

The molecular formula of the compound can be determined by finding the number of atoms of each element in a molecule and combining them to form the molecular formula.From the percent composition, we can find the number of moles of each element in 100 g of the compound.

40 g of Carbon, which is equal to 40/12 = 3.33 moles of Carbon

6.7 g of Hydrogen, which is equal to 6.7/1 = 6.7 moles of Hydrogen

53.3 g of Oxygen, which is equal to 53.3/16 = 3.33 moles of Oxygen

The molar mass of the compound is 90 amu, so there are 90 g/mol of the compound.The molecular formula can be determined by dividing the number of moles of each element by the smallest number of moles of the elements, then rounding to the nearest whole number.

Carbon: 3.33 moles / 3.33 moles = 1

Hydrogen: 6.7 moles / 3.33 moles = 2

Oxygen: 3.33 moles / 3.33 moles = 1

Therefore, the molecular formula for the compound is C1H2O1 or COH2.

Hope this helps! Correct me if I’m wrong.