Q < K

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Labiba Sardar 2A
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Joined: Sat Jul 20, 2019 12:15 am

Q < K

Postby Labiba Sardar 2A » Sat Jan 18, 2020 11:44 am

When Q < K, is saying "the reaction proceeds to the right" the same thing as saying "the reaction proceeds to form products"?

Rebekah Alfred 1J
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Re: Q < K

Postby Rebekah Alfred 1J » Sat Jan 18, 2020 12:04 pm

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").

605395381
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Re: Q < K

Postby 605395381 » Sat Jan 18, 2020 12:25 pm

When Q < K, that means the reaction is not in equilibrium and the reaction is favoring the product side.

CMaduno_1L
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Re: Q < K

Postby CMaduno_1L » Sat Jan 18, 2020 2:17 pm

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!

Sanjana Borle 2K
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Re: Q < K

Postby Sanjana Borle 2K » Sat Jan 18, 2020 3:22 pm

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.

Daniel Chen 2L
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Re: Q < K

Postby Daniel Chen 2L » Sat Jan 18, 2020 5:11 pm

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.

Michelle Xie 2B
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Re: Q < K

Postby Michelle Xie 2B » Sat Jan 18, 2020 5:47 pm

When Q is less than K, more products tend to form.

Betania Hernandez 2E
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Re: Q < K

Postby Betania Hernandez 2E » Sun Jan 19, 2020 12:10 am

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.

805097738
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Re: Q < K

Postby 805097738 » Sun Jan 19, 2020 12:21 pm

correct that is what that means. forward rxn favors the product

Robert Tran 1B
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Re: Q < K

Postby Robert Tran 1B » Sun Jan 19, 2020 12:48 pm

Yes, because in a chemical equation, the products are on the right side. Thus, a shift to the right means more products will form.

Bryce Barbee
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Joined: Wed Sep 18, 2019 12:20 am

Re: Q < K

Postby Bryce Barbee » Sun Jan 19, 2020 1:08 pm

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.

Areena H 2K
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Re: Q < K

Postby Areena H 2K » Sun Jan 19, 2020 2:08 pm

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.

IScarvie 1E
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Re: Q < K

Postby IScarvie 1E » Sun Jan 19, 2020 9:59 pm

Yes, when a reaction proceeds to the right, it forms products

Jesalynne 2F
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Joined: Wed Sep 18, 2019 12:18 am

Re: Q < K

Postby Jesalynne 2F » Sun Jan 19, 2020 10:04 pm

When Q<K you have more reactants, so more products form.

Nuoya Jiang
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Re: Q < K

Postby Nuoya Jiang » Sun Jan 19, 2020 10:20 pm

Yes, it is. The product side is favoured.

Long Luong 2H
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Joined: Thu Sep 19, 2019 12:16 am

Re: Q < K

Postby Long Luong 2H » Sun Jan 19, 2020 10:35 pm

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!

Nare Nazaryan 1F
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Joined: Fri Aug 09, 2019 12:17 am

Re: Q < K

Postby Nare Nazaryan 1F » Sun Jan 19, 2020 10:50 pm

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.


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