Analysis of vitamin $C$ shows that it contains $40.92 %$ carbon by mass, $4.58 %$ hydrogen and $54.50 %$ oxygen. Determine the empirical formula of vitamin $C$ .

Open in App

Solution

Vitamin $C$ contains $40.92 %$ carbon by mass, $4.58 %$ hydrogen and $54.50 %$ oxygen.

100 g of vitamin $C$ will contain 40.92 g C, 4.58 g, H and 54.50 g O.
Atomic masses of C, H and O are 12 g/mol, 1 g/mol and 16 g/mol respectively.

Number of moles of $C = \frac{40.92 g}{12 g / m o l} = 3.4 m o l$ .

Number of moles of $H = \frac{4.58 g}{1 g / m o l} = 4.58 m o l$ .

Number of moles of $O = \frac{54.50 g}{16 g / m o l} = 3.40 m o l$ .

Mole ratio of C : H : O = 3.4 : 4.58 : 3.4 = 3 : 4 : 3

Empirical formula of vitamin $C$ is $C_{3} H_{4} O_{3}$ .

Suggest Corrections

Similar questions

C, 38.71 %

H, 9.67 %

38.71 %

9.67 %

C, 38.71 %

H, 9.67 %

C - 75 %

H - 25 %

Join BYJU'S Learning Program