Acompound contains only carbon, hydrogen, and oxygen. combustion of 9.612 mg of the compound yields 14.41 mg co2 and 3.93 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.)

Formula used for determining the number of moles:

number of moles = -(1)

Mass of = 14.41 mg (given)

Mass of = 3.93 mg (given)

Number of moles of from =

=

Number of moles of from =

=

Mass of carbon  =

=

Mass of hydrogen =

=

Mass of oxygen = total mass of the compound - mass of carbon- mass of hydrogen

=

=

Now, number of moles of oxygen =

=

To identify the empirical formula; divide the number of moles of carbon, hydrogen and oxygen with least number of moles.

Thus,

Now, multiply the numbers with 3 to get the hydrogen number in whole number, we get

The empirical formula =

The empirical weight =

=

Divide the molecular weight with empirical weight to find the factor between empirical formula and molecular formula  , we get

=

=

Now, multiply the numbers of carbon, hydrogen and oxygen with 2 to get molecular formula, we get

Number of carbon = 6

Number of hydrogen = 8

Number of oxygen = 6

Thus, molecular formula is .

a: 45.9 meters

b: 4.29 seconds

step-by-step explanation:

a: h(t)=1/2(-9.8)(3)^2+0(3)+90

h(t)=-4.9(3)^2+90

h(t)=-44.1+90

h(t)=45.9 meters

b: 0=1/2(-9.8)(t^2)+0t+90

0=-4.9t^2+90

-90=-4.9t^2

18.37=t^2

t=4.29 seconds

in the second question, the numbers aren't exact, but they're a close approximation.

atomic mass = 39

number of neutrons = 20

number of protons= 19

electronic configuration = 1s2 2s2 2p6 3s2 3p6 4s1

the number of electron in first shell = 2

number of electrons in n=3 shell = 8