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Postby megangeorge-1K » Thu Jan 17, 2019 10:30 pm

when Q<K, will more products form because the forward reaction is favored?

Lauren Ho 2E
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Re: Q<K

Postby Lauren Ho 2E » Thu Jan 17, 2019 10:45 pm

Yes! Here is a visual representation of that:
AAAWUWG0.jpg (15.09 KiB) Viewed 80 times

Faith Fredlund 1H
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Re: Q<K

Postby Faith Fredlund 1H » Thu Jan 17, 2019 10:46 pm

Yes. When Q<K, the forward reaction is favored, so this means reactants will be used up to form more products. Taking product out of a solution such that it never reaches equilibrium is a method many chemical/ drug manufacturing companies will utilize so that they will obtain higher total outputs of product.

Albert Duong 4C
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Re: Q<K

Postby Albert Duong 4C » Thu Jan 17, 2019 10:49 pm

Q and K are ratios of product to reactants. Essentially, if Q<K, then there is initially a higher ratio of reactants to products than when at equilibrium, so that means in order for Q to have the same product to reactant ratio as K, more products must be made to offset the higher reactant ratio. The forward reaction is thus favored.

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Re: Q<K

Postby chrisavalos-2L » Sat Jan 19, 2019 11:20 pm

Yes, when Q<K the forward reaction is favored and therefore in order to reach equilibrium as all reactions attempt in the long run, there will be more products formed to eventually reach equilibrium.

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