An unknown organic compound (0.315 g) containing only c, h, and o produces 0.771 of co2 and 0.105 g of h2o when it undergoes complete combustion. the approximate molar mass is 108 g/mol. which of the following compounds could be the identification of the unknown?

C₆H₄O₂

Explanation:

Given parameters:

Mass of the unknown compound = 0.315g

Atoms contained in the compound C, H and O

Mass of CO₂ produced = 0.771g

Mass of H₂O = 0.105g

Molar mass of compound = 108gmol⁻¹

The complete combustion of most hydrocarbon compounds like this would produce carbon dioxide and water only.

Solution

We first find the mass of the Carbon, hydrogen and Oxygen in the compounds given.

Mass of carbon in compound = x mass of CO₂

Molar mass of C = 12

Molar mass of CO₂ = 12 + (16x2) = 44

Mass of CO₂ produced = 0.771g

Mass of carbon in compound =   x 0.771=0.2103g

Mass of H in compound =   x mass of H₂O

Molar mass of H in H₂O = 2

Molar mass of H₂O = 2 + 16 = 18

Mass of H₂O = 0.105g

Mass of H in compound =   x 0.105 = 0.012g

Now, to find the mass of oxygen in the compound, we sum the mass H and C and subtract from the mass of the compound given:

Mass of oxygen = 0.315 - (0.2103 + 0.012)= 0.0927g

We then continue to derive the empirical formula of the compound.

                                    C                       H                         O

mass of

atoms                      0.2103                0.012                   0.0927

Moles                  0.2103/12             0.012/1                 0.0927/16

                               0.018                   0.012                    0.006

Dividing by

the smallest       0.018/0.006       0.012/0.006           0.006/0.006

                                   3                           2                                1

The empirical formula of the compound is C₃H₂O

From the empirical formula, we can find the compound from the given molar mass:

Molecular formula = (Empirical formula)n

Where n is the number of repeating times of the empirical formula present in one mole of the molecule.

Therefore n =

 Molar mass of the empirical formula C₃H₂O = (12x3) + (2x1) + (16) = 54g/mol

               n = = 2

The molecular formula of the compound is = 2(C₃H₂O) = C₆H₄O₂

its going to be mutualism cuz they both benefit from the relationship.

~batmans wife dun dun

> b takes place in the gas phase in an isothermal tubular reactor. the feed is one mole of a per one mole of c, an inert. the entering temperature and pressure are 427°c and 10 atm, respectively. the gas constant r = 0.08206 atm · l/mol · k.