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the position of a reaction relative to equilibrium
A catalyst cannot change the equilibrium position. However, it can change its rate.
Equilibrium in chemistry is the point or position at which the rate of the forward reaction is equal to the rate of the reverse reaction. Whatever concentrations exist at this point are referred to as equilibrium concentrations.
The value of the equilibrium constant K is only influenced by temperature.
temperature, pressure (in the case of gases), concentration
the position of a reaction relative to equilibrium
A catalyst cannot change the equilibrium position. However, it can change its rate.
With the position of equilibrium of this reaction, it is almost unable to carry out the backward reaction.
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.
The forward and backward reactions are equal.
Equilibrium is pushed to the reactant side
The temperature of a reaction will entirely change th equilibrium position for any given reaction. If I'm right, as you increase the temperature, the equilibrium shifts closer to the endothermic reaction as there is more heat to consume. It may also, of course, change other properties of the substances involved in the reaction, but that depends on the chemicals.
Equilibrium in chemistry is the point or position at which the rate of the forward reaction is equal to the rate of the reverse reaction. Whatever concentrations exist at this point are referred to as equilibrium concentrations.
The reactants concentration is equal to products concentration.
The value of the equilibrium constant K is only influenced by temperature.
temperature, pressure (in the case of gases), concentration
It depends on the order of the reaction. If it is zero order, decreasing the reactant concentration will have NO effect on the rate. If it is 1st or 2nd order (or more), then decreasing the concentration will DECREASE the reaction rate.