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### Reaction Direction

Posted: Sun Jan 12, 2020 9:01 pm
How do we determine is the reaction is "left" or "right". And does the direction of the reaction matter if it is composition or decomposition?

### Re: Reaction Direction

Posted: Sun Jan 12, 2020 9:06 pm
The left and right portions are arbitrary, as, given a reversible reaction, you could switch both sides and the left directional reaction would now be the new right directional compound

### Re: Reaction Direction

Posted: Sun Jan 12, 2020 9:07 pm
You determine it by comparing the equilibrium constant (K) with the reaction quotient (Q). If Q is less than K, then there are less products so the reaction is going to the right. If Q is greater than K, then there are more products so the reaction is going to the left. In this case, it doesn't matter what type of reaction it is.

### Re: Reaction Direction

Posted: Sun Jan 12, 2020 9:09 pm
If Q>K then the reaction moves to the left because the concentration of products is greater than the concentration of reactants so the reaction would move towards the side of the reactants to reach equilibrium. If Q<K, then the reaction moves to the right because the concentration of reactants is greater than the concentration of products so the reaction would move towards the side of the products to reach equilibrium.

### Re: Reaction Direction

Posted: Sun Jan 12, 2020 9:30 pm
I know that K represents the equilibrium constant, but what does Q represent in this situation?

### Re: Reaction Direction

Posted: Sun Jan 12, 2020 9:31 pm
How do you solve for Q in this situation?

### Re: Reaction Direction

Posted: Sun Jan 12, 2020 9:46 pm
005384106 wrote:I know that K represents the equilibrium constant, but what does Q represent in this situation?

In this situation, Q would represent the state of the reaction at a point where equilibrium has not been reached yet. This is why they are asking about which direction the reaction will occur ("left" or "right") because the Q value will determine it.

### Re: Reaction Direction

Posted: Sun Jan 12, 2020 11:12 pm
I am confused with the equilibrium ratio when using molarity values compared to the equilibrium ratio using partial pressure. Can someone please explain this to me. Thank you

### Re: Reaction Direction

Posted: Sun Jan 12, 2020 11:38 pm
When dealing with equilibrium, the reactions are typically reversible meaning that it could be left to right or the other way around

### Re: Reaction Direction

Posted: Tue Feb 04, 2020 9:14 pm
Morgan Carrington 2H wrote:
005384106 wrote:I know that K represents the equilibrium constant, but what does Q represent in this situation?

In this situation, Q would represent the state of the reaction at a point where equilibrium has not been reached yet. This is why they are asking about which direction the reaction will occur ("left" or "right") because the Q value will determine it.

How will I know whether a reaction will occur left or right based on Q?

### Re: Reaction Direction

Posted: Wed Feb 05, 2020 10:27 am
005384106 wrote:
Morgan Carrington 2H wrote:
005384106 wrote:I know that K represents the equilibrium constant, but what does Q represent in this situation?

In this situation, Q would represent the state of the reaction at a point where equilibrium has not been reached yet. This is why they are asking about which direction the reaction will occur ("left" or "right") because the Q value will determine it.

How will I know whether a reaction will occur left or right based on Q?

If Q>K the reaction will move to the left because the concentration of products is greater than the concentration of reactants. If Q<K the reaction will move to the right because the concentration of reactants is greater than the concentration of products.The reaction will move towards the direction necessary to reach equilibrium.

### Re: Reaction Direction

Posted: Wed Mar 11, 2020 6:24 pm
What is the reaction quotient, Q? Can you determine it by concentration values or K?

### Re: Reaction Direction

Posted: Sun Mar 15, 2020 6:56 am
One way to determine if the reaction will proceed right or left is by comparing to equilibrium value to the reaction quotient value. If your reaction quotient (Q) is less than K than your reactants will continue to react and your reaction will proceed to the right towards the products and vice versa, if Q is greater than K then the reaction will favor going left towards the reactants.

### Re: Reaction Direction

Posted: Sun Mar 15, 2020 1:09 pm
Compare Q and K

### Re: Reaction Direction

Posted: Wed Mar 18, 2020 1:01 am
You can determine them using Q and K, for Q>K, the reaction favors reactants and moves left, for Q<K, it favors products and proceeds to the right.