Question: What Condition Must Be Satisfied So That Q K?

What is Q and K in equilibrium?

Q is a quantity that changes as a reaction system approaches equilibrium.

K is the numerical value of Q at the “end” of the reaction, when equilibrium is reached..

Which side of equilibrium is favored?

The side of lower energy is favored at equilibrium. By favored we mean there is a higher concentration. Acid base reactions are reversible and therefore equilibrium reactions.

What does Q represent in chemistry?

The reaction quotient (Q) measures the relative amounts of products and reactants present during a reaction at a particular point in time. The reaction quotient aids in figuring out which direction a reaction is likely to proceed, given either the pressures or the concentrations of the reactants and the products.

What’s the difference between Q and K?

The difference between K and Q is that, K is the constant of a certain reaction when it is in equilibrium, while Q is the quotient of activities of products and reactants at any stage of a reaction. Therefore, by comparing Q and K, we can determine the direction of a reaction.

What is the difference between K and K?

A second side note about K is that pure solids and pure liquids don’t get included in it. Their concentrations are so big that we can just take them as being constant throughout the reaction….Summary of the differences between K and k:KLittle kThermodynamic, not kineticKinetic, not thermodynamic6 more rows

How do I calculate k?

Calculating K from Known Initial Amounts and the Known Change in Amount of One of the SpeciesWrite the equilibrium expression for the reaction.Determine the molar concentrations or partial pressures of each species involved.Determine all equilibrium concentrations or partial pressures using an ICE chart.More items…

What is the relationship between Q and K?

Q can be used to determine which direction a reaction will shift to reach equilibrium. If K > Q, a reaction will proceed forward, converting reactants into products. If K < Q, the reaction will proceed in the reverse direction, converting products into reactants. If Q = K then the system is already at equilibrium.

What happens if Q is less than K?

We compare Q and K to determine which direction the reaction will proceed to obtain equilibrium. If Q is greater than K, the system will shift to the left. If Q is less than K, the system will shift to the right. If Q is equal to K than the system is already at equilibrium so it will not shift in either direction.

What is the difference between the reaction quotient Q and the equilibrium constant K?

K is the equilibrium constant. Therefore K is revealing the amount of products to reactants that there should be when the reaction is at equilibrium. Q is used to determine whether or not the reaction is at an equilibrium.