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a-The equilibrium will shift toward the products. b-The equilibrium will shift toward the reactants. c-Keq will increase. d-Keq will decrease. e-There will be no shift in equilibrium.
why do you think it's E
it was kind of a guess but if it cant increase or decrease it cant be C or D, but E just looked like the best guess to me, im not to good in chem :/
well @bransonsmommy it will have an effect. think about it like this the reaction is already at equilibrium, so there's a certain amount of reactants and products at equilibrium for this reaction. if we add more on one side, we call that a stress, the reaction has to adjust to that stress. follow so far?
somewhat, i'm leaning towards A, but i am still a little fuzzy on this...
not really.. im doing online classes and they give us no notes or anything..
when you have a reaction, say you have a bridge right? the products are on one side the reactants are on the other. the reaction will proceed until it reaches a point where the rate of forward reaction = the rate of the reverse reaction, that's equilibrium a little analogy here is the number of cars going back and forth is the same. Equilibrium does not mean that the concentrations of the reactants and products are equal. Can you see why? Also what is favored in this reaction, reactants or products? at equilibrium |dw:1443623016742:dw|
i think i kinda get it a little better, so the answer would be B?
yeah i would say so
but there's a lot to be learned here at least @bransonsmommy, sometimes they give you Keq value and sometimes they dont for this question they didn't. like if i gave you a keq of 10^6 at 25 C what type of reaction is this? how do you know what does it favor?