You can use physical methods to separate a mixture and also some chemical methods too.
Mixture is just a physical combine.
However a compound is a chemical combine so you must use special methods to separate it
Is there suppose to be a picture? Cause I do t see one
but where Is the volume in order for us to determine the concentration. since we have moles in H+ ions
then you can say
concentration = M*1000/V
Make an observation.
Conduct research.
Form hypothesis.
Test hypothesis.
Record data.
Draw conclusion.
Replicate.
One thing that is designed to change in the set up of the experiment. ( The things that I can change) Independent Variable.
Answer:
The answer to the question is
The pressure of carbon dioxide after equilibrium is reached the second time is 0.27 atm rounded to 2 significant digits
Explanation:
To solve the question, we note that the mole ratio of the constituent is proportional to their partial pressure
At the first trial the mixture contains
3.6 atm CO
1.2 atm H₂O (g)
Total pressure = 3.6+1.2= 4.8 atm
which gives
3.36 atm CO
0.96 atm H₂O (g)
0.24 atm H₂ (g)
That is
CO+H₂O→CO(g)+H₂ (g)
therefore the mixture contained
0.24 atm CO₂ and the total pressure =
3.36+0.96+0.24+0.24 = 4.8 atm
when an extra 1.8 atm of CO is added we get Increase in the mole fraction of CO we have one mole of CO produces one mole of H₂
At equilibrium we have 0.24*0.24/(3.36*0.96) = 0.017857
adding 1.8 atm CO gives 4.46 atm hence we have
(0.24+x)(0.24+x)/(4.46-x)(0.96-x) = 0.017857
which gives x = 0.031 atm or x = -0.6183 atm
Dealing with only the positive values we have the pressure of carbon dioxide = 0.24+0.03 = 0.27 atm
