Q vs K
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Re: Q vs K
Q is for when the reaction isn't at equilibrium. K is for when the reaction is at equilibrium.
Re: Q vs K
Q and K are similar in that they are calculated in the same way, Q = [P]/[R] and K = [P]/[R].
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Re: Q vs K
The difference between Q and K is that K is the equilibrium constant which in other words is when the reaction has reached equilibrium. Q, the reaction quotient, is something you can do during anytime of the reaction. By comparing Q to K, you can see the direction of the reaction. If Q=K, then you know equilibrium has been reached.
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Re: Q vs K
Additionally, if
- Q<K, the reaction will proceed forward to create more products
- Q>K, the reaction will proceed in reverse to create more reactants
- Q<K, the reaction will proceed forward to create more products
- Q>K, the reaction will proceed in reverse to create more reactants
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Re: Q vs K
Q and K are essentially the same when it comes to calculating them. The difference is that K is the value when the reaction is at equilibrium while Q can be found at anytime during the reaction to see if the action is at equilibrium or not.
Can someone please explain to me how to ask a question on Chem Community. I cannot figure it out. Thanks
Can someone please explain to me how to ask a question on Chem Community. I cannot figure it out. Thanks
Re: Q vs K
The reason why the reaction moves forward when the reaction quotient (Q) is less than the equilibrium constant (K) is because the lesser value means that there is less product than there should be when the reaction reaches equilibrium and thus more product is needed, so the reaction moves forward. As for when Q is greater than K, the reaction moves in the reverse direction because there is now more product than there is at equilibrium and thus you need to move backwards.
Re: Q vs K
Q is not at equilibrium, it is just products over reactants at any given time during the reaction. K is the equilibrium constant of the products over her reactants.
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Re: Q vs K
K is an equilibrium constant, while Q is a reaction quotient. K is found when the reaction is at equilibrium, but Q can be calculated at any time during the reaction. You can compare the reaction quotient, Q, to the equilibrium constant, K, to determine the direction of the reaction.
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