No they do not.
A catalyst is a thing (atom, molecule, element, etc.) that speeds up a chem. rxn by lowering the activation energy without being altered itself. So it only cause the reaction to occur faster, but will not have any affect on the equilibrium. Also, since the catalyst is not altered, it should 'come out' exactly as it 'went in.'
A catalyst does not affect the value of the equilibrium constant (Keq) of a reaction. The presence of a catalyst increases the rate of both the forward and reverse reactions equally, allowing the system to reach equilibrium more quickly but does not change the final equilibrium composition.
The catalyst will accelerate the forward and reverse reactions equally, therefore not changing the position of the equilibrium. This results in the system reaching a new equilibrium faster but with the same concentrations of reactants and products as before the catalyst was added.
Equilibrium position. The catalyst speeds up the rate at which equilibrium is reached by lowering the activation energy for both the forward and reverse reactions equally. The concentrations of reactants and products at equilibrium remain the same.
Catalysts do not change the postition of the reaction's equilibrium. Adding a catalyst will increase the rate of reaction, but it will do this by providing another pathway for the reaction to occur acros, meaning a lower activation enthalpy is needed. :)
When a catalyst is added to a chemical reaction, the rate of the reaction will increase without being consumed in the process. This means that the reaction will reach equilibrium faster and require less activation energy. The overall chemical equilibrium and products formed will remain the same.
A catalyst does not affect the value of the equilibrium constant (Keq) of a reaction. The presence of a catalyst increases the rate of both the forward and reverse reactions equally, allowing the system to reach equilibrium more quickly but does not change the final equilibrium composition.
The catalyst will accelerate the forward and reverse reactions equally, therefore not changing the position of the equilibrium. This results in the system reaching a new equilibrium faster but with the same concentrations of reactants and products as before the catalyst was added.
Equilibrium position. The catalyst speeds up the rate at which equilibrium is reached by lowering the activation energy for both the forward and reverse reactions equally. The concentrations of reactants and products at equilibrium remain the same.
Equilibrium constant changes when temperature changes. For an endothermic reaction, the equilibrium constant increases with temperature while for an exothermic reaction equilibrium constant decreases with increase in temperature. Equilibrium constants are only affected by change in temperature.
By definition a catalyst cannot affect equilibrium because although a catalyst can speed up a chemical reaction, it cannot change the thermodynamics of it, and equilibrium is determined solely by thermodynamics. A catalyst may help a system reach equilibrium more quickly, but it will not change it. One possible way a catalyst could affect equilibrium is by introducing a catalyst that affects a different reaction involving the substrate or products of the original reaction, but this would be cheating since the system would no longer be closed.
Adding a catalyst to the mixture would not affect the equilibrium concentration of H2O. A catalyst speeds up the rate of the forward and reverse reactions equally, without changing the position of the equilibrium. This means that the equilibrium concentration of H2O would not be affected by the presence of a catalyst.
If demand decreases and supply is constant, the price will increase.
The correct answer is a simple one: The system is unaffected by a catalyst in a system in equilibrium.
Catalysts do not change the postition of the reaction's equilibrium. Adding a catalyst will increase the rate of reaction, but it will do this by providing another pathway for the reaction to occur acros, meaning a lower activation enthalpy is needed. :)
When a catalyst is added to a chemical reaction, the rate of the reaction will increase without being consumed in the process. This means that the reaction will reach equilibrium faster and require less activation energy. The overall chemical equilibrium and products formed will remain the same.
To reach equilibrium faster, you can increase the concentration of reactants, raise the temperature (if it's an endothermic reaction), decrease the volume (for gases), or use a catalyst to speed up the reaction rate. It's important to remember that altering these factors can only help reach equilibrium faster, not change the position of the equilibrium itself.
A catalyst cannot change the equilibrium position. However, it can change its rate.