Answer: one simple distillation column is required to separate the stream into five pure products. With four different flat bottom flask, for collection of the distilled products
Explanation: simple distillation works with the difference in boiling points of the liquid to be separated. For the separation of five different constituent to be possible, we have to know the boiling points of the constituents.
For your understanding, let's define constituents in the liquid to be A, B, C, D, E. And the boiling points increases respectively. Start by heating the liquid to the boiling point of A to extract A. After a while check if the constituents A is still dropping in the flat bottom flask, if it has stopped dropping, it simply means that we have extracted all A constituents in the liquid, label the Flask A. Get another flask to extract constituent B.
Heat the mixture to the boiling point of B, after a while check if constituent B is still dropping in the flat bottom flask, if it has stopped dropping,it means that we have extracted all B constituent in the liquid, label the Flask B. Get another flask for C.
Repeat the same process for C and D.
After Extracting D we don't need to distillate E because we already have a pure form of E inside to the conical flask.
SEE PICTURE TO UNDERSTAND WHAT A SIMPLE DISTILLATION LOOKS LIKE
<span>It takes 3 breaths to get to 1.2 l. One breath is then (1.2 l) / 3 breaths = .4l/breath.
To get to 3.0 l we need the difference from 1.2 l.
3.0-1.2 = 1.8 l.
Divide the difference by liters/breath (.4) to get how many needed breaths.
(1.8 l)/(.4 l/breath) = 4.5 breaths to get the balloon to 3.0 l.
In total there were 3 breaths+ 4.5 breaths = 7.5breaths to get to 3.0 l.
To find the total moles multiply 7.5breaths by .060 moles/breath
7.5 breaths*.060moles/breath = .45moles</span>
During this phase Change heat energy is being absorbed by the molecules, and as a result the molecules possess a greater ability to move around and possess higher kinetic energy because of this. The molecules also possess a higher potential energy.
So 100 g
of this substance has 63.57 g of carbon, 6 g of hydrogen, 9.267 of nitrogen,
and 21.17 of oxygen.
I need to
have them all in moles (n). You can find the molar mass (M) of each element in
a periodic table.
n = m/M
63.57 g C
-> 63.57 g C/12.01 g/mol = 5.29 moles C
6 g H
-> 6 g C/1.008 g/mol = 5.95 moles H
9.267
g N -> 9.267 g N/14.01 g/mol = 0.6615 moles N
21.17
g O -> 21.17/16.00 g/mol = 1.32 moles O
So
the minimum formula has this rate:
C
5.29 H 5.95 N 0.6615 O 1.32
Now you should divide all those numbers by
the smallest one (1.32):
C 4 H 4.5 N 0.5 0 1
Now it looks a lot more like a molecular
formula… but we still have fractions.
Let’s multiply all numbers by 2:
C8H9N1O2
<span>Now they are all whole numbers!
</span>
So the minimum formula
is C8H9NO2
The minimum
formula is not always equal to the molecular formula… but in this case, I found
there is a molecular formula with this same numbers, and it’s called acetaminophen.
Answer: The standard enthalpy of formation of liquid octane is -250.2 kJ/mol
Explanation:
The given balanced chemical reaction is,
First we have to calculate the enthalpy of reaction 
.
![\Delta H^o=[n_{O_2}\times \Delta H_f^0_{(O_2)}+n_{H_2O}\times \Delta H_f^0_{(H_2O)}]-[n_{C_8H_{18}}\times \Delta H_f^0_{(C_8H_{18})+n_{O_2}\times \Delta H_f^0_{(O_2)}]](https://tex.z-dn.net/?f=%5CDelta%20H%5Eo%3D%5Bn_%7BO_2%7D%5Ctimes%20%5CDelta%20H_f%5E0_%7B%28O_2%29%7D%2Bn_%7BH_2O%7D%5Ctimes%20%5CDelta%20H_f%5E0_%7B%28H_2O%29%7D%5D-%5Bn_%7BC_8H_%7B18%7D%7D%5Ctimes%20%5CDelta%20H_f%5E0_%7B%28C_8H_%7B18%7D%29%2Bn_%7BO_2%7D%5Ctimes%20%5CDelta%20H_f%5E0_%7B%28O_2%29%7D%5D)
where,
We are given:
Putting values in above equation, we get:
![-1.0940\times 10^4=[(16\times -393.5)+(18\times -285.8)]-[(25\times 0)+(2\times \Delat H_f{C_8H_{18}(l)}]](https://tex.z-dn.net/?f=-1.0940%5Ctimes%2010%5E4%3D%5B%2816%5Ctimes%20-393.5%29%2B%2818%5Ctimes%20-285.8%29%5D-%5B%2825%5Ctimes%200%29%2B%282%5Ctimes%20%5CDelat%20H_f%7BC_8H_%7B18%7D%28l%29%7D%5D)
Thus the standard enthalpy of formation of liquid octane is -250.2 kJ/mol
