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Postby 605110118 » Thu Jan 09, 2020 3:12 pm

How does the reactant quotient relates to K?

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Joined: Wed Sep 11, 2019 12:17 am

Re: Q

Postby vanessas0123 » Thu Jan 09, 2020 3:14 pm

Q is used at any point of the reaction, while K is calculated when the rxn is at equilibrium.
If Q<K, then the forward reaction will proceed (to make more products).
If Q> K, then the reverse reaction will proceed.

Kate Osborne 1H
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Re: Q

Postby Kate Osborne 1H » Thu Jan 09, 2020 3:15 pm

The reaction quotient can be compared to K to find out if the reaction is in pre-equilibrium (Q<K), equilibrium(Q=K), or post-equilibrium(Q>K).

Connie Chen 1E
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Re: Q

Postby Connie Chen 1E » Thu Jan 09, 2020 3:18 pm

The reaction quotient is a ratio of the concentration of products to reactants when the system has not yet reached equilibrium. If Q<K, the forward reaction will be favored in order to create more product because there are not enough products in relation to reactants for the system to be at equilibrium. If Q>K, the system will favor the reverse reaction to create more reactant because there is not enough reactant in relation to products for the system to be at equilibrium.

Izzie Capra 2E
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Re: Q

Postby Izzie Capra 2E » Thu Jan 09, 2020 3:38 pm

I think Q is especially important in a lab setting because you can predict which direction a reaction will proceed, even if it is not at equilibrium. You can calculate Q at any point during a reaction, but K is only at equilibrium. Comparing the values will show you where you "are" in a chemical reaction.

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