A 5.41 g sample of carbon reacts with hydrogen to form 6.32 g of an organic compound. What is the empirical formula of the organic compound?

CH₂

Explanation:

From the question given above, the following data were obtained:

Mass of Carbon (C) = 5.41 g

Mass of compound = 6.32 g

Empirical formula =?

Next, we shall determine the mass of Hydrogen (H) in the compound. This can be obtained as follow:

Mass of Carbon (C) = 5.41 g

Mass of compound = 6.32 g

Mass of Hydrogen (H) =?

Mass of H = mass of compound – mass of C

Mass of H = 6.32 – 5.41

Mass of H = 0.91 g

Finally, we shall determine the empirical formula of the compound. This can be obtained as follow:

Mass of C = 5.41 g

Mass of H = 0.91 g

Divide by their molar mass

C = 5.41 / 12 = 0.451

H = 0.91 / 1 = 0.91

Divide by the smallest

C = 0.451 / 0.451 = 1

H = 0.91 / 0.451 = 2

Thus, the empirical formula for the compound is CH₂

the seeing the electronic configuration we can say that the element is fluorine.

fluorine is the most electronegative element in the periodic table.

but by only seeing the configuration we cannot say about its reactivity because we don't know if its configuration after excitation or by addition of electrons.

but if not then, it is the lightest halogen and exists as a highly toxic pale yellow diatomic gas at standard conditions. as the most electronegative element, it is extremely reactive: almost all other elements, including some noble gases, form compounds with fluorine.