## Calculating Q

Hannah Yates 1K
Posts: 59
Joined: Fri Sep 28, 2018 12:27 am

### Calculating Q

When do you calculate Q? I am having some trouble understanding why you would need this and when to use it.

ian_haliburton_1f
Posts: 61
Joined: Fri Sep 28, 2018 12:24 am

### Re: Calculating Q

You calculate Q when you are not sure whether the reaction is at equilibrium. If you already know the reaction’s K value, you can use the same formula for K at any time, even when the reaction is not at equilibrium, and call the calculated value Q. Its value relative to K (whether it is less than K or greater than K) helps you to predict the future dynamics of the reaction. For example, if you calculate a Q that is less than K, you can infer that the reaction will then favor product formation over reactant formation to get closer to to the equilibrium state.

Danielle_Gallandt3I
Posts: 70
Joined: Fri Sep 28, 2018 12:24 am

### Re: Calculating Q

Q uses the same equation as K, but it can be calculated at any point of the reaction, whereas K can only be calculated at equilibrium. You can then compare Q to K to find out where the reaction is relative to equilibrium and which way the reaction might favor.

Zubair Ahmed 1L
Posts: 81
Joined: Fri Sep 28, 2018 12:16 am

### Re: Calculating Q

Both Q and K use the same equation during calculation. However, K is used at equilibrium while Q can be used at any point during a reaction. It is important understand the fact that Q can be changed due to changes in pressure and concentration but K does not. K shifts only when there is a change in temperature.

Katie_Duong_1D
Posts: 69
Joined: Fri Sep 28, 2018 12:27 am

### Re: Calculating Q

You can calculate Q exactly how you would calculate K. Q = [products]/[reactants]. If Q<K, the reaction shifts right to reach equilibrium. If Q = K, the reaction is at equilibrium. If Q >K, the reaction shifts left.

Cynthia Aragon 1B
Posts: 47
Joined: Mon Apr 09, 2018 1:38 pm

### Re: Calculating Q

For Q, we can plug in the concentrations of reactants/products at any instant of time. By comparing Q with K, we can predict whether the reaction will move in the forward or reverse direction. If Q< K the reaction will proceed in the forward direction. If Q>K, the reaction will proceed in the reverse direction and if Q=K the reaction is already at equilibrium.

Andrew Bennecke
Posts: 62
Joined: Fri Sep 28, 2018 12:15 am

### Re: Calculating Q

The Reaction Quotient (Q) is similar to the Equilibrium Constant (K) in that they are calculated the same way. However, Q only equals K when at equilibrium, it is somewhat like a "temporary" K value. You would need to calculate Q whenever the system is not in equilibrium, or you are unsure whether or not the system is stable.

Katelyn Pham 4E
Posts: 30
Joined: Fri Sep 28, 2018 12:21 am

### Re: Calculating Q

You calculate the reaction quotient (Q) when you are determining which direction the reaction shifts. Q=[Products]/[Reactants] just as K. If Q<K then the reaction shifts right to form towards products and if Q>K then the reaction shifts left to form towards the reactants.

Brian Hom 2F
Posts: 60
Joined: Fri Sep 28, 2018 12:24 am

### Re: Calculating Q

You calculate Q when the reaction has been disrupted from equilibrium. Q is similar to K except Q is used to tell which direction the reaction will proceed in order to reach equilibrium.

Vana Mirzakhani 3I
Posts: 62
Joined: Fri Sep 28, 2018 12:24 am

### Re: Calculating Q

Put simply, Q is calculated when the reaction is not at equilibrium.

Posts: 57
Joined: Fri Sep 28, 2018 12:27 am

### Re: Calculating Q

Q is calculated whenever the equation is not at equilibrium, so if there is a change or anything similar. Also, Q is calculated whenever you are trying to see the result of the reaction (i.e. if the reaction favors the reactants or products).

Mikka Hoffman 1C
Posts: 62
Joined: Fri Sep 28, 2018 12:23 am
Been upvoted: 2 times

### Re: Calculating Q

You can calculate Q at any point in the reaction and it will tell you if the reaction is at equilibrium and, if not, which direction the reaction will proceed.