In this video you are going to learn how
to find a compound's molecular formula.
Alright let's do this.
Hello hello Melissa
Maribel here and I help students like you
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So what is an empirical formula versus a
molecular formula? Great question, an
empirical formula is an educated guess
or an approximation as to how many
elements are within that compound. It is
by no means the exact chemical formula.
The exact chemical formula is the
molecular formula. So in order to figure
out a molecular formula, you first have
to figure out your empirical formula.
Let's try one.
Nicotine has a molar mass
of a 162.1 grams per mole
and a composition of 74.0% of carbon, 8.70% of hydrogen
and 17.30% of nitrogen. Find the molecular formula.
To find the molecular formula you first
have to figure out what your empirical
formula is. So our first step is to
change our percentage to grams. To do so
note that if we were to add up all of
these percentages it would be out of
100%. So because it's out of 100%
there is no need to
multiply or convert anything. You are
literally changing your percentage to
grams. These will be our new values that
we'll use in the next step. Step two is
to convert your grams that we found in
our previous step to moles. When
converting to grams to moles we use
molar mass of each element to get to
moles. So in our case we'll have the
seventy four point zero grams of carbon,
align that with the molar mass of carbon
which is 12.01 grams. Those grams would
cancel and then we'll get our
6.1615 moles of carbon. We'll
do the same thing for hydrogen except
aligning hydrogen's
molar mass on the bottom and then we'll
divide and you get 8.613 moles of hydrogen. And lastly we'll
do the same exact thing for nitrogen
except nitrogen's molar mass is
14.01. Divide these values and
you get 1.234 moles
of nitrogen. The next step is to then
divide by the smallest number of moles.
Which in our case will be the nitrogen.
Divide each one of these values and your
moles would cancel and we're left with
the new subscripts of our empirical
formula. Now we have our empirical
formula, those subscripts that we found
in the previous step are as shown and
now it's on to figure out our molecular
formula. So the next step is to figure
out the molar mass of this empirical
formula. Start with your carbon which we
have 5 of them and multiply by the
individual molar mass of carbon.
We'll get 60.05. Do the
same for hydrogen. Now there are 7
times that 1.01 and you
get 7.07. But there's
only 1 nitrogen so you don't even have
to really multiply. It's 1 times
14.01 which is itself.
We'll add all these values together and
your molar mass of your empirical
formula gives you 81.13 grams per mole. Your next step
is to divide. You will be dividing your
molecular formulas molar mass, divided by
the empirical formula's molar mass. In the
initial question you were given the
molecular formula's molar mass. You will
always be given that because there is no
other way to figure out the molecular
formula without the molecular formula's
molar mass. We found our empirical
formula's molar mass and a nice little
trick for you to remember that molecular
formula's molar mass goes on top and the
empirical formula's molar mass goes on
the bottom is, "please oh please don't
forget about ME." ME molecular formula on
top, empirical formula's molar mass on the
bottom. So we'll divide those two values
in our case and these grams per mole
will cancel
and you get a whole number of 2.
Our final step is to multiply that whole
number which was 2 that we found in
the previous step, to each subscript of
your empirical formula. So in the black
you'll see our empirical formula. We're
multiplying by two that we found before.
And finally we get our molecular formula
of C 10 H 14 and N 2. This is the exact
chemical formula of nicotine.
Let's test out what you just learned.
I know these questions are a lot of
steps but the more you practice the
easier it's gonna become and you're
gonna remember all the little steps.
So if you have to rewatch this video, if you
have to just keep practicing over and
over, you will pass chemistry, it's really
just about practice. But if you need some
more help check the description box
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