Answer !

what is the molecular formula of the compound that contains 18.18 w/w% hydrogen and 81.82 w/w% carbon and its relative density referred to carbon dioxide is 1.000?

The osmotic pressure will allow us to calculate the molar mass of the substance:

π = iMRT

2.13 atm = (a) (x / 0.175 L) (0.08206 L atm / mol K) (298 K)

x = 0.015243 mole

2.04 g / 0.015243 mole = 133.83 g/mole

For your problem, let us calculate the amount of carbon and hydrogen. Then, by subtraction, we will check for oxygen.

carbon: 36.26 g x (12.011 g / 44.01 g) = 9.8959 g

hydrogen: 14.85 g x (2.016 g / 18.015 g) = 1.6618 g

oxygen: 22.08 minus (9.8959 + 1.6618) = 10.5223 g

Calculate moles of each element:

carbon: 9.8959 g / 12.011 /mol = 0.8239 mol

hydrogen: 1.6618 g / 1.008 g/mol = 1.6486 mol

oxygen: 10.5223 g / 15.999 g/mol = 0.657685 mol

Determine a molar whole number ratio:

carbon: 0.8239 / 0.657685 = 1.25

hydrogen: 1.6486 / 0.657685 = 2.5

oxygen: 0.657685 / 0.657685 = 1

Look at it like this:

carbon: 1.25 = 5/4 = 5

hydrogen: 2.5 = 10/4 = 10

oxygen: 1 = 4/4 = 4

C5H10O4

the answer would be a

the electron configuration that you gave me has 16 electrons ergo it has 16 protons ergo it is the element sulfur.