Acompound contains only carbon, hydrogen, and oxygen. combustion of 11.75 mg of the compound yields 17.61 mg co2 and 4.81 mg h2o. the molar mass of the compound is 176.1 g/mol. what are the empirical and molecular formulas of the compound? (type your answer using the format co2 for co2.)

Number of moles is defined as the ratio of given  mass in g to the molar mass.

First, convert the given mass of carbon dioxide in mg to g:

1 mg = 0.001 g

17.61 mg = 0.01761 g

Number of moles of carbon dioxide =

=

Mass of carbon  = number of moles of carbon dioxide \times molar mass of carbon

=

=

Number of moles of water=

=

Since, water contains two hydrogen atoms. Thus,

Moles of hydrogen =

=

Mass of hydrogen =

=

Mass of oxygen =

=

Number of moles of oxygen =

=

Now,

Divide the smallest number to get the whole number,

we get,

Now, multiply all the subscript by 3 to get the whole number,

  (empirical fomula)

Molar mass of the compound  =

=

Divide given molar mass of the compound with the molar mass of the compound.

=

=

Thus, multiply the subscripts of empirical formula by 2 to get the molecular formula, we get:

Hence, empirical formula is and molecular formula is

adding or remove a gaseous reactant or product changes the concentrations. if the concentration of reactant or product is increased, the system will shift away from the side in which concentration was increased (i.e. if the concentration of reactants is increased, the system will shift toward the products. if more products are added, the system will shift to form more reactants). conversely, if the concentration of reactant or product is decreased, the system will shift toward the side in which concentration was decreased (i.e. if reactants are removed, the system will shift to form more reactants. if the concentration of products is decreased, the equilibrium will shift toward the products).

explanation:

i think it is true since you can test the answer and can use observations to complete it.