How does qc differ from kc

Qc and Qp are the ratio of the concentrations or partial pressures of a system at a specific point at which the forward and reverse reactions are occurring. It has not yet reached equilibrium, so it will be different from K. If Q is equivalent to K, then that "point" is equilibrium. K determines the ratio of product over reactant at equilibrium and the value should be the same for each reaction under the same conditions and temperature.

Q is very similar to K as they are calculated the same way with using products over reactants of the reaction. Press ESC to cancel. Ben Davis May 31, What does it mean when Qc is greater than KC? How does QC compare to KC? When QC KC a reaction will? What happens if you increase temperature in equilibrium? What is the KC equation? What is KC affected by? What is the value of KC? Why is KC only affected by temperature? What happens to KC when volume increases? Is KP equal to KC?

Should KC values be the same? Do you include water in KC? What happens to equilibrium constant when reaction is doubled? What happens to K when reaction is reversed? Which equilibrium constant value indicates that the reverse reaction is favored? Can KC be negative? Is KC affected by concentration? Can the equilibrium constant ever be zero? What does a positive equilibrium constant mean? What does a higher equilibrium constant mean? What does the equilibrium constant depend on? What does it mean when the equilibrium constant is less than 1?

How do you know if a product is reactant or favored? How can you tell if a forward or reverse reaction is favored? If not, which direction will the reaction progress to reach equilibrium? As a system approaches towards equilibrium, Q approaches towards K. K: What Does It Mean? To properly predict which way a reaction will progress, you must know these relationships. Handy Chart Outlining the Relationships of Q and K Remembering these simple relationships will aid you to solving for the progression of a reaction.

Predicting the Shift of a Reaction Without Calculations Depending on what a problem asks of you, sometimes it is unnecessary to make any calculations at all. Take, for example, the reaction below: If you start with 4. Solutions 1 The reactions shifts to the left, towards the reactants.

The reaction will shift to the right. The reaction will shift to the left. References Alberty, R. Cornish-Bowden, et al. Chem 66 : — Gold, J.