We learned Le Chatelier's principle which is, "if a system at equilibrium is disturbed by a change in temperature, pressure, or the concentration of one of the components, the system will shift its equilibrium position so as to counteract the effect of the disturbance".
Kc=[C]c[D]d [A]a[B]b
This equation is used to find the equilibrium constant of molar concentration in an equation.
Kp=(C)c(D)d(A)a(B)b
This equation is used to find the equilibrium constant of partial pressures of each gas in an equation.
Kp=Kc(RT)Δn
This equation is used to convert from Kc to Kp. The delta n means the number of moles on the product side, minus the number of moles on the reactant side. Q gives the same ration as K, but for a system that is not at equilibrium. Q is calculated using the initial concentrations of the reactants and products. If
Qc < Kc, there is more reactant and less product in the initial conditions than at equilibrium. The reaction will then move towards the products, so to the right. If Qc > Kc, there is less reactant and more product in the initial conditions than at equilibrium. The reaction will then move towards the reactants, so to the right. If Q = K, the reaction is already at equilibrium under initial conditions so it doesn't shift.
Another way used to calculate equilibrium is using a RICE chart. RICE stands for Reaction, Initial, Change, and at Equilibrium. With some reactions, they may end up getting into cube roots. However, if x is smaller than 5% of initial concentrations, it can be left out and the quadratic can be avoided.
A reaction is favorable when ΔG° is less than 0, and is called exergonic. A reaction is unfavorable when ΔG° is greater than 0, and is called endergonic. ΔG° for a reaction measures the difference between the free energies of the reactants and products when all components of the reaction are present at standard-state conditions. When it's negative, the reaction would have to shift to the right converting some of the reactants into products. There is only one value of ΔG° at a given temperature, but an infinite number of values of ΔG. The smaller the value of ΔG°, the closer the standard state is to equilibrium. The larger the value of ΔG°, the further the reaction has to go to reach equilibrium.
This week I'd give my understanding about an 8.5. I was able to do the lecture quizzes without any confusion, and although I missed Monday I completed the equilibrium I worksheet. This unit I've also paid a lot of attention to the lectures and in class, and I'm really trying to do as well on this test as I did on the last one. I think the worksheets have really been helping understand the concepts and Concept tests as well. I hope I do even better on this test than on the Gases unit because I think I really understand and like the topic of equilibrium. I find it interesting and the demonstrations at the beginning of class are intriguing and useful to learning the topic.
This week I'd give my understanding about an 8.5. I was able to do the lecture quizzes without any confusion, and although I missed Monday I completed the equilibrium I worksheet. This unit I've also paid a lot of attention to the lectures and in class, and I'm really trying to do as well on this test as I did on the last one. I think the worksheets have really been helping understand the concepts and Concept tests as well. I hope I do even better on this test than on the Gases unit because I think I really understand and like the topic of equilibrium. I find it interesting and the demonstrations at the beginning of class are intriguing and useful to learning the topic.
