K and Q

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K and Q

Postby ClaireHW » Thu Mar 15, 2018 8:56 pm

In terms of a redox reactions, what do K and Q equal?
Do they equal [red]/[ox] or [ox]/[red]?


Claire Woolson Dis 1K

Gurvardaan Bal1L
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Re: K and Q

Postby Gurvardaan Bal1L » Thu Mar 15, 2018 10:09 pm

I don't think they would be any different, K and Q are basically the same thing just that K is at equilibrium and Q is at a particular time in a reaction.

The formula for that would be the concentrations of products multiplied against each other(each raised to the power of their respective coefficients) divided by the same thing on the bottom except now with the concentrations of the reactants and their own coefficient exponents.

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