Reaction Quotient

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Reaction Quotient

Postby TiffanyL1G » Wed Jan 09, 2019 6:37 pm

What is the reaction Quotient and how does one solve for that? For example in the 6th edition textbook, problem number 13a, how would you solve for that problem?

Emma Scholes 1L
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Re: Reaction Quotient

Postby Emma Scholes 1L » Wed Jan 09, 2019 6:41 pm

The Reaction Quotient is calculated the same way that K is calculated. The equation is Q=[Products]/[Reactants]. The reaction quotient is used to determine which direction the reaction will proceed.

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Re: Reaction Quotient

Postby Heesu_Kim_1F » Wed Jan 09, 2019 7:07 pm

The reaction quotient (Q) measures the amount/concentration of products and reactants at a given time, as opposed to K, which is equal to the value of Q only at equilibrium. One solves Q in the same way as one does K. Thus, for problem 11.13a, Q = 1/((P BCl3)^2). This is because Hg is liquid and B2Cl4 and Hg2Cl2 are solids, meaning they won't factor into the reaction quotient. Hope this helps!

Nina Do 4L
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Re: Reaction Quotient

Postby Nina Do 4L » Wed Jan 09, 2019 7:09 pm

From what was gathered in lecture, the quotient reaction is the values anytime during the reaction, not necessarily at equilibrium. So not only does it determine which way the reaction goes, but if the value of Q is not equal to K then you can tell that it is not at equilibrium.

If Q < K, the forward reaction is favored.
If Q > K, the reverse reaction is favored.

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Re: Reaction Quotient

Postby deepto_mizan1H » Wed Jan 09, 2019 8:14 pm

The reaction quotient also may not always match with the equilibrium constant, which should also be checked for when doing the problem. It'll probably come up later on in the quarter.

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