1) chromatography- separation by inner molecular attractions.
2) distillation- separation by boiling point differences.
3) filtration- separation by particle size
4) crystallization- separation by solubility
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The mass percent of potassium chloride is 1.386%
<u><em>calculation</em></u>
mass percent = actual mass/ Theoretical mass x 100
Actual mass = 9.35 g
Theoretical mass is calculated as below
Step 1 : write the equation for reaction
KCl + H₂O → KOH + HCl
Step 2: find the moles of H₂O
moles = mass÷ molar mass
The molar mass of H₂O = (2 x1 ) +(16) = 18 g/mol
moles is therefore = 162.98 g÷ 18 g/mol =9.054 moles
Step 3: use the mole ratio to determine the moles of KCl
KCl: H₂O is 1:1 therefore the moles of KCl is also = 9.054 moles
Step 4: find the theoretical mass of KCl
mass = moles x molar mass
from periodic table the molar mass of KCl = 39 +35.5 =74.5 g/mol
mass = 9.054 moles x 74.5 g/mol =674.5 g
Theoretical mass is therefore = 9.35 g/ 674.5 g x 100 = 1.386%
Answer: Equilibrium constant is 0.70.
Explanation:
Initial moles of 
= 0.35 mole
Volume of container = 1 L
Initial concentration of 
Initial moles of 
= 0.40 mole
Volume of container = 1 L
Initial concentration of 
equilibrium concentration of 
[/tex]
The given balanced equilibrium reaction is,
Initial conc. 0.35 M 0.40M 0 0
At eqm. conc. (0.35-x) M (0.40-x) M (x) M (x) M
The expression for equilibrium constant for this reaction will be,
![K_c=\frac{[CO_2]\times [H_2O]}{[CO]\times [H_2O]}](https://tex.z-dn.net/?f=K_c%3D%5Cfrac%7B%5BCO_2%5D%5Ctimes%20%5BH_2O%5D%7D%7B%5BCO%5D%5Ctimes%20%5BH_2O%5D%7D)
we are given : (0.35-x)= 0.18
x = 0.17
Now put all the given values in this expression, we get :
Thus the value of the equilibrium constant is 0.70.
