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Q < K

Posted: Sat Jan 18, 2020 11:44 am
by Labiba Sardar 2A
When Q < K, is saying "the reaction proceeds to the right" the same thing as saying "the reaction proceeds to form products"?

Re: Q < K

Posted: Sat Jan 18, 2020 12:04 pm
by Rebekah Alfred 1J
When Q < K at some time during the reaction, then [R] > [P] and the forward reaction is favored (which is the same thing as saying it "proceeds towards the products" and "proceeds to the right").

Re: Q < K

Posted: Sat Jan 18, 2020 12:25 pm
by 605395381
When Q < K, that means the reaction is not in equilibrium and the reaction is favoring the product side.

Re: Q < K

Posted: Sat Jan 18, 2020 2:17 pm
by CMaduno_1L
A method I use to remember the meanings of when Q>K and Q<K is to think of Q wanting to approach K. This can be visualized as a number line with K placed in the center. If Q is less than K, then the reaction must proceed in the forward direction in order to reach K. Conversely, if Q is greater than K, then the reaction must occur in the reverse direction in order to reach equilibrium. Hope this helps!

Re: Q < K

Posted: Sat Jan 18, 2020 3:22 pm
by Sanjana Borle 2K
If Q is less than K, then it means that there are more reactants than products when compared to equilibrium, so more products need to be formed.

Re: Q < K

Posted: Sat Jan 18, 2020 5:11 pm
by Daniel Chen 2L
When Q is less than K it means that the reaction hasn't gone all the way through yet, and is not at equilibrium. It is more shifted to the right side.

Re: Q < K

Posted: Sat Jan 18, 2020 5:47 pm
by Michelle Xie 2B
When Q is less than K, more products tend to form.

Re: Q < K

Posted: Sun Jan 19, 2020 12:10 am
by Betania Hernandez 2E
Yes, both statements mean the same thing. When Q<K, there is more reactants than products and it is not at equilibrium. In order for it to get to equilibrium, the reaction proceeds to the right to form products.

Re: Q < K

Posted: Sun Jan 19, 2020 12:21 pm
by 805097738
correct that is what that means. forward rxn favors the product

Re: Q < K

Posted: Sun Jan 19, 2020 12:48 pm
by Robert Tran 1B
Yes, because in a chemical equation, the products are on the right side. Thus, a shift to the right means more products will form.

Re: Q < K

Posted: Sun Jan 19, 2020 1:08 pm
by Bryce Barbee
Yes this is what that means. If Q is less than K, then the reaction still needs to form more products at a higher rate than it is going towards reactants.

Re: Q < K

Posted: Sun Jan 19, 2020 2:08 pm
by Areena H 2K
If K is greater than Q that means that at point during the reaction, there are more reactants that are forming and to reach equilibrium the reaction proceeds to the right which is saying that more products are formed.

Re: Q < K

Posted: Sun Jan 19, 2020 9:59 pm
by IScarvie 1E
Yes, when a reaction proceeds to the right, it forms products

Re: Q < K

Posted: Sun Jan 19, 2020 10:04 pm
by Jesalynne 2F
When Q<K you have more reactants, so more products form.

Re: Q < K

Posted: Sun Jan 19, 2020 10:20 pm
by Nuoya Jiang
Yes, it is. The product side is favoured.

Re: Q < K

Posted: Sun Jan 19, 2020 10:35 pm
by Long Luong 2H
I like to think about K on a number line. If Q is less than K, it is to the left of K and is trying to go right (towards products). If Q is greater than K, it is to the right of K and trying to go left (towards products). I hope this helps!

Re: Q < K

Posted: Sun Jan 19, 2020 10:50 pm
by Nare Nazaryan 1F
Yes, it is the same because when Q is less than K, there are more reactants than products so the reaction needs to form more products to reach equilibrium.