shifts left or right

[Agustina Santa Cruz 2F]

Hi, I know that when Q<K then its a forward reaction and it shift right. It shifts left when it is the opposite. But, what exactly does this shift indicate? I know it's important to know whether it is a forward or reverse reaction but what is the importance of identifying the shift?

[Sean Wang 1F]

The equation shifting to the right means that the reaction is more inclined to form products. The equation shifting to the left means that the reaction is more inclined to form reactants.

[Rose_Malki_3G]

If the equation is shifting to the left, it means it will produce more reactants. If the equation is shifting to the right, it means it will produce more products

[Kaylee Messick 3J]

The shift would indicate which way the reaction is going to go in order to be at equilibrium again. More reactants or products will form depending on the value of Q, which is important because the value of Q can be at anytime during the reaction, so comparing this value to K will indicate which direction the reaction will go to reach equilibrium. Hope this helps!

[AlyssaMaynard1C]

Hi, I know that when Q<K then its a forward reaction and it shift right. It shifts left when it is the opposite. But, what exactly does this shift indicate? I know it's important to know whether it is a forward or reverse reaction but what is the importance of identifying the shift?

Do we always need to use the Q or are there some problems where you don't need it?

[Joshua Chung 2D]

If a reaction is shifting to the left, then it will begin to produce more reactants relative to products. If it is shifting to the right, then it will produce more products relative to reactants.

[Julianna_flores3E]

Hi, I know that when Q<K then its a forward reaction and it shift right. It shifts left when it is the opposite. But, what exactly does this shift indicate? I know it's important to know whether it is a forward or reverse reaction but what is the importance of identifying the shift?

Do we always need to use the Q or are there some problems where you don't need it?

The equation of Q is the same as K so when it is clear that the reaction is at equilibrium technically you do not need Q because it will equal K.

[josephspindler2H]

Shifting to the right means that the products are favored (more will be produced to fit the equilibrium) while shifting to the left means the reactants are favored (again more will be produced). It can helpful to think of the products being on the right side of the chemical equation while the reactants are on the left. It's important to remember that these shifts are highlighting a return to equilibrium after some kind of disturbance.

[Ethan Goode 2H]

If it is inclined to shift right, then more products will be easily formed, and vice versa if going left.

[sabrina ghalambor 2J]

shifting to the left favors reactant production, and shifting to the right favors product production!

[jasonfarrales3D]

Hello! When a reaction "shifts to the right," this shows that the formation of products is favored (there are more reactants than products in the reaction, and in order to get back to the K value, the production of product is heavily needed). When the reaction "shifts to the left," this indicates that the formation of reactants is favored (there are more products than reactants in the reaction, and in order to get back to the K value, the production of reactant is heavily needed).

[Lauren Sarigumba 1K]

When Q>K, then the reaction will favor the reactants (reverse reaction). If Q<K, then the reaction will favor the products (forwards reaction).

[Neel Bonthala 2G]

The shift just refers to the amount of product formed versus the amount of reactant! A shift to the left means more reactant is formed at equilibrium, while a shift to the right means there will be more product formed at equilibrium instead.

[David Y]

If shifts right, more products being produced.

[Britney Tran IJ]

when the reaction shifts right, the production of products is being favored.

[jasmineculilap_3F]

A shift to the left means that reactants are favored while a shift to the right favors products.

[Justin Zhang_1A]

A shift to the left or right determines whether reactants or products are favored, which tells you if there is more product or reactant formed.

[Charisma Arreola 2F]

The shift indicates which side is favored (product or reactants).

[Wasila Sun 2I]

If it helps, shifts left or right don't actually mean the reaction is moving. Shifts only indicate whether the reactants or products will be favored going forward.

[Maddie Turk Disc 2J]

All it means is that the equation is going to be favoring the forward reaction, so products will be forming. Nothing is physically shifting.

[Melanie Lin 3E]

Hi! When Q<K, it means that the denominator (or reactants) increased and vice versa. So when there's more reactants, the equilibrium will shift towards the right to form more products. Hope this helps!

[AlyssaMaynard1C]

shifting to the left favors reactant production, and shifting to the right favors product production!

Do we do these tests to figure out where the reaction is shifting then? Is this the only way to tell?

[SamayaJoshi1A]

The shift indicates whether more products or reactants are being made in the reaction. Most of teh time, the reaction is heading towards the equilibrium, where a set amount of products and reactants are being formed.

[NayeliPlayas_1L]

If the reaction shifts right then more products will be formed and if the reaction shifts left then more reactants will be formed.