i supplied their percentage masses split by each element"s relative atomic mass then separated thru by the smallest mole proportion.

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moles of carbon= #19.36/12=1.613# moles of hydrogen= #3.25/1=3.25#moles of oxygen= #77.39/16=4.8369#

divide thru through the smallest ratio

C #1.613/1.613#H #3.25/1.613#O #4.8369/1.613#

=CH2O3


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The empirical formula is the SIMPLEST entirety number ratio specifying constituent facets in a types...


Just like all these difficulties, the usual rigmafunction is to assume a #100*g# mass and also then interrogate the molar quantities of each aspect.

#"Moles of hydrogen,"# #(3.25*g)/(1.00794*g*mol^-1)=3.220*mol.#

#"Moles of carbon,"# #(19.36*g)/(12.011*g*mol^-1)=1.612*mol.#

#"Moles of oxygen,"# #(77.39*g)/(16.00*g*mol^-1)=4.84*mol.#

And we divide thru by the SMALLEST molar quantity to acquire the empirical formula...

#"Empirical formula"-=C_((1.612*mol)/(1.612*mol))H_((3.220*mol)/(1.612*mol))O_((4.84*mol)/(1.612*mol))-=CH_2O_3#


Answer link
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Meave60
Feb 27, 2018

The empirical formula is #"CH"_2"O"_3"#.


Explanation:

An empirical formula represents the lowest whole number ratio of aspects in a compound. Tright here are several actions involved.

1. Determine the moles of each facet by splitting its given mass by its molar mass. When percentages add as much as 100%, we can directly convert percent to mass in grams.

2. Determine the mole ratios in between each facet and also the lowest variety of moles by dividing the moles of each element by the lowest variety of moles. This action determines the subscripts for the aspects.

3. If all mole ratios are totality numbers, you have actually the lowest whole number ratio and have the right to write them as subscripts for the compound.

4. If one or more mole proportion is not a whole number, then all ratios must be multiplied by a element that will make all ratios entirety numbers.

Moles of elements

Due to the fact that molar mass is a portion (g/mol), I favor to divide by the molar mass by multiplying by its reciprocal (mol/g). I think it provides what happens via the systems more clear.

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#"H":# #3.25color(red)cancel(color(black)("g H"))xx(1"mol H")/(1.008color(red)cancel(color(black)("g H")))="3.22 mol H"#

#"C":# #19.36color(red)cancel(color(black)("g C"))xx(1"mol C")/(12.011color(red)cancel(color(black)("g C")))="1.61 mol C"#

#"O":# #77.39color(red)cancel(color(black)("g O"))xx(1"mol O")/(15.999color(red)cancel(color(black)("g O")))="4.84 mol O"#

Mole ratios

Because moles cancel and also mole ratios are dimensionless, I am not going to label the moles.