Determining The Favored Side of an Equilibrium Product

[Bronson Mathos 1H]

Hello, I may be missing something from my notes but I know that when determining which direction the reaction is proceeding in an equilibrium question we solve for Q, but I was wondering if someone could tell me the basis we use to state the direction of the reaction based on this Q?

[Stuti Pradhan 2J]

If Q is less than K, then the equilibrium shifts to the right or makes more products. On the other hand, if Q is greater than K, then the equilibrium shifts to the left or makes more reactants. This is because if Q is less than K, that means there is currently a higher concentration of reactants than there is at equilibrium, which increases the denominator, making Q smaller. Therefore, to reach equilibrium, the reaction needs to produce more products. The opposite is true when Q is greater than K. If Q is larger, that means there is currently a higher concentration of products than there is at equilibrium, which increases the numerator of Q. To reach equilibrium from here, more reactants would have to be formed.

Hope this helps!

[Megan Singer 3D]

To figure this out all you have to do is think about how Q = [P]/[R]. If Q > K, the [P] is higher/the [R] is lower in Q than it is in K, so [P] goes down and [R] goes up (reactants are favored). If Q < K, the [R] is higher/the [P] is lower in Q than it is in K, so [R] goes down and [P] goes up (products are favored).

[Natalie 3k]

I'm not fully sure if this is what you're asking, but to find the direction of the reaction we have to compare the Q value to K. If Q is bigger than K then it shifts to the left (because it is measured by products/reactants, and a number bigger than K would mean there are more products), and if Q is less than K it would shift to the right (because there are more reactants than at equilibrium). Hope this helps !

[Katie Phan 1K]

If Q < K, the reaction will shift to the right (towards products).. If Q > K, the reaction will shift to the left (towards reactants). If they are equal, the reaction is at equilibrium.

[edward_brodell_2I]

To avoid confusion I always put Q left and K right and the direction of the inequality determines which gets favored Q<K inequality sign is right so products are favored etc.

[Jarrett Sung 3B]

You have to compare the Q value to the K equilibrium constant, and if Q < K, the reaction will proceed towards the products while if Q > K, the reaction will proceed towards the reactants. If Q = K, the reaction is at equilibrium.

[Kelly Tran 1J]

If Q < K, the equilibrium will shift to the right and products are favored. If Q > K, the equilibrium will shift to the left and reactants are favored.

[Pratika Nagpal]

does it matter how much less than or more than K, Q is.

like is there a particular threshold after which we can determine whether products or reactants will be favoured ?

[Karina Grover 1A]

If Q is less than K, then that means that there are more reactants. If there are more reactants, then the reaction will want to proceed in the forward direction to make more products. Thus, product formation is favored.

If Q is greater than K, then that means that there are more products. If there are more products, then the reaction will want to proceed in the reverse direction to make more reactants. Thus, reactant formation is favored.

[Sean Wang 1F]

If Q is less than K, then products are favored because the numerator needs to increase. If Q is greater than K, then reactants are favored because the denominator needs to increase.

[AlbertGu_2C]

The way I remember it is when looking at Q >,<, or = K, the way the open end of the sign is facing is which side is favored.

[Taha 2D]

If Q is less than K, then the equilibrium shifts to the right or makes more products. On the other hand, if Q is greater than K, then the equilibrium shifts to the left or makes more reactants.