Here is the problem:
PCl3(g) + Cl2(g) <==> PCl5(g) Kc = 26 at 275K
all in a 6.40 L flask
PCl3: .1 mol
Cl2: .1 mol
PCl5: .01 mol
Assuming ideal gas conditions, What is the Kp, Qp, and
the shift of direction? (if someone can help me
set up this problem that would be great!)
where
Now assuming ideal behavior of PCl3 , Cl2 and PCl5 , we can calculate their individual partial pressures as,
Given,
Hence,
Now. we can calculate Qp (which is reaction quotient in terms of pressure),
From above analysis, it is clear that Kp > Qp which indicates that the net reaction proceeds to right direction i.e. the shift of direction towards the right side of the reaction.
Here is the problem: PCl3(g) + Cl2(g) <==> PCl5(g) Kc = 26 at 275K all in...
For this reaction: PCl3(g) + Cl2(g) <==> PCl5(g) Kc = 26 at 275K Initially, you have 0.10 mol PCl3, 0.10 mol Cl2, and 0.010mol PCl5 all in a 6.40L flask. Assuming ideal gas conditions, calculate: Kp, Qp, and state which direction the reaction will shift.
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