A quantity that characterizes the position of equilibrium for a reversible reaction; its magnitude is equal to the mass action expression at equilibrium. K varies with temperature.
Dont u mean what is equilibrium?
If the demand shift to the right, the equilibrium price and quantity will shift from the initial equilibrium price and quantity to the next, i mean the equilibrium price and quantity will increase as compare to the first.
It means that all forces acting on it are equal.
No
Total amounts of products and reactants are not changing.-- Apex
Cooling the equilibrium mixture will shift the equilibrium towards the side favoring the formation of the reactants (endothermic direction). The intensity of the mixture color could decrease if the reactants are colorless or have a lighter color compared to the products.
The system will rebalance.
A numerically large equilibrium constant (Keq) indicates that the equilibrium lies far to the right, with more products present at equilibrium than reactants. This means that the forward reaction is favored, leading to a higher concentration of products compared to reactants in the equilibrium state.
To ensure that you have the more product which will be produced because the equilibrium will shift to produce it. This will produce heat and also more chemical product that you want in the equilibrium mixture.
Dont u mean what is equilibrium?
The equilibrium will be re-established.
If you remove H½ from the mixture, the equilibrium will shift to the left to compensate for the loss, meaning more H½O will dissociate to reform some of the missing H½. This will increase the concentration of H½O in an attempt to restore equilibrium.
Solids do not affect the equilibrium of a chemical reaction because their concentration remains constant and does not change during the reaction. Only the concentrations of gases and dissolved substances in a reaction mixture can affect the equilibrium position.
A small equilibrium constant (Kc) typically indicates that the reaction tends to favor the reactants at equilibrium rather than the products. This suggests that the reaction is not proceeding to a significant extent in the forward direction.
Adding reactants to an equilibrium mixture will cause the equilibrium to shift to the right in order to consume the excess reactants. This helps restore the equilibrium conditions by favoring the forward reaction to produce more products.
Two half arrows are usually used to denote a reaction which is in equilibrium. If they are the same length to one another then equilibrium is obtained and you have a mixture of reagent and product. If the arrow pointing right is larger then this denotes that the reaction is predominently a forwards reaction and favours the product and vice versa.
when a system is in equilibrium it is stable and all its parts function smoothly