Chemical Equilibria and Reaction Quotients

Many chemical reactions don't just go one way, they go forwards and backwards. Once there is balance between the two, this is an equilibrium. And we need to be able to predict how much stuff there will be at equilibrium! Get ready to bust out those ICE boxes, folks.
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[@ProfessorDaveExplains]

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Hey, great tutorial! It really helped me to understand species concentrations better than my textbook. Just a small point though...at around 3:32, you mentioned that for Kc >> 1, "...we are creating more products..." which is not *technically* correct. The forward reaction is favored (when Kc >> 1), but at equilibrium, reactant and product concentrations are approximately constant. Making more products only occurs when the system is not in equilibrium, for Kc >> 1 and as you mentioned, when Kc > Q. It's a small point, but the semantic distinction is quite significant for a student to grasp chemical equilibrium. I know that you understand this distinction, but thought I would mention it here so other people don't leave with the idea of more products being *created* when Kc >> 1. I've subscribed and will be checking out your other videos. Your explanations are so clear and easy to follow. Thanks! :)

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question Equilibrium does mean the rate of the forward reaction is equal to the rate of the reverse reaction Equilibrium constant = forward reaction / backward reaction If equal, it means one Why does the reaction reach the equilibrium state? The equilibrium constant is not one?

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[@1NikkiPink1]

Hi professor Dave. Thanks again for the great videos. Quick question on the checking comprehension. Did you multiply both sides by negative one to get to the quadratic form? When I multiply both sides by the denominator, I get the opposites for addition and subtraction.

[@ProfessorDaveExplains]

nope i just brought the left side to the right side! if you have 0.036 - 0.36x and you bring it to the other side to be with 4x^2, you have to subtract the number and add the x term so the signs reverse.

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in 2:52 why did he only take away one (0.135) form the 1m instead of two? shouldn't the product be 0.730 as both reactants have 0.135. someone please explain

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That's because the coefficient of the Pcl5 was one. Both pcl3 and pcl2 come from one mole of Pcl5 so it is only subtracted by a single x

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Professor Why we raise the concentration with the power of their stoichiometric coefficients??

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[@shashankshekhar1266]

Hey Professor Christ. Suppose If I take the equation of PCl5 PCl3 and Cl2 at 1:44 . Now, since Kc(equilibrium constant) is independent of initial concentration, I can take Z molar solution and should still get the same answer. But if initial concentration is Z and degree of dissociation is a , Kc comes out to be (Za)^2/(Z-Za) => Za^2/(1-a). That is, it depends on Z(initial concentration) . PLEASE HELP.

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[@dr.bucci.]

Thank you very much this is extremely helpful. However, I am confused about how you got 4x^2 in the numerator when solving for X using the Equilibrium Constant Expression. Could you explain why we use 4x^2 instead of 2x^2? Thanks again!

[@ProfessorDaveExplains]

you have to square the 2 as well!

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Hello, On the checking comprehension why is [NO2]^2 changed to 4x^2 and not 2x^2? Is it because of the equation give?

[@ProfessorDaveExplains]

don't forget that when you do (2x)^2 the exponent operates on both the 2 and the x! so it becomes (2^2)(x^2) or 4x^2

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