Reaction Quotient Q c pridicts the direction of reaction. All rights reserved. Classscience » Chemistry. Share with your friends. Li, Y. Drew, Coord. Download references. You can also search for this author in PubMed Google Scholar. Correspondence to Yue Liu. Reprints and Permissions. J Math Chem 52, — Download citation. Received : 06 July Accepted : 19 January Published : 13 February Issue Date : May Anyone you share the following link with will be able to read this content:.
Sorry, a shareable link is not currently available for this article. Provided by the Springer Nature SharedIt content-sharing initiative. Skip to main content. Remember that the concentrations of liquids and solids do not change, so they are excluded from the expression. On the other hand, a small amount of products small numerator divided by a large value for the concentration of reactants large denominator would result in a small value for Q.
The value of K c at K is As a result, some of the reactants will become products, causing the reaction to shift to the right. To decrease the amount of products, the reaction will shift to the left and produce more reactants. Remembering these simple relationships will aid you to solving for the progression of a reaction.
A chart outlining them can be found below. Depending on what a problem asks of you, sometimes it is unnecessary to make any calculations at all. Take, for example, the now familiar reversible reaction listed below :. What do you think will happen if more of the product, methanol CH3OH , is added?
In order to re-establish equilibrium, the reaction will progress to the left, towards the reactants. This means some of the added methanol will break down into carbon monoxide and hydrogen gas. Now, what if more of the reactants, carbon monoxide and hydrogen gas, are a? You should realize that this would upset the equilibrium.
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