Question

2) A 1.00 g sample of vitamin C contains C, H, and O and is combusted to produce 1.50 g of CO₂ and 0.41 g of H₂O.

Find the empirical formula of vitamin C. If the molecular mass of vitamin C is 176.12 g/mol, what is the molecular formula?

Answer 1

Answer:The empirical formula for this vitamin : C₃H₄O₃

Further explanation

The empirical formula is the smallest comparison of atoms of compound =mole ratio of the components

The principle of determining empirical formula

Determine the mass ratio of the constituent elements of the compound.

Determine the mole ratio by dividing the percentage by the atomic mass

Mass of C in CO₂ :(MW C = 12 g/mol, CO₂=44 g/mol)

Mass of H in H₂O :(MW H = 1 g/mol, H₂O = 18 g/mol)

Mass O = Mass sample - (mass C + mass H) :

mol ratio C : H : O =

Step-by-step explanation: