Q<K

[megangeorge-1K]

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

[Lauren Ho 2E]

Yes! Here is a visual representation of that:

[Faith Fredlund 1H]

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]

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.

[chrisavalos-2L]

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.