Which of the following will change the value of equilibrium constant?Change in amount of catalystChange in concentration of reactantChange in pressureChange in temperature (2024)

FAQs

Which of the following changes will change the value of the equilibrium constant? ›

Equilibrium constants are not changed if you add (or change) a catalyst. The only thing that changes an equilibrium constant is a change of temperature. The position of equilibrium is not changed if you add (or change) a catalyst. A catalyst speeds up both the forward and back reactions by exactly the same amount.

The only thing that affects equilibrium constant is the change in temperature.

The equilibrium constant is only changed by changing the temperature of the reaction because this changes the way the reaction proceeds because it changes which compounds are the most stable and therefore are favored by the reaction.

Catalyst does not affect the position of equilibrium and hence it does not have any effect on the value of equilibrium constant. only change in temperature can change the equilibrium constant.

The factors affecting equilibrium constant are temperature, pressure, and concentration. While there is no change in equilibrium constant on change of pressure and concentration, an increase in temperature leads to a decrease in concentration and vice versa.

Chemical equilibrium will shift towards the reactant when the concentration of product increases,less product is formed and the concentration of reactant increases as the concentration of product decreases.

Hence, change in pressure or concentration of reactants does not affect equilibrium. The addition of catalyst also does not affect equilibrium.

1- equilibrium constant depends on temperature. hence changing the temperature will change the value of equilibrium constant.

Equilibrium constants are temperature-dependent, independent of reaction quantities, catalysts, and inert materials. Moreover, it is independent of concentrations, pressures, or volumes of reactants. The temperature dependence of the equilibrium constant is generally determined by of the reaction.

The equilibrium constant is dependent only on temperature only not on the other parameters such as concentration, pressure, etc. so the equilibrium constant is constant when the reaction is doubled.

How do the following changes affect the value of the equilibrium constant for a gas-phase exothermic reaction? ›

For a gas-phase exothermic reaction, a decrease in temperature will cause the equilibrium to shift to the side that produces heat (the exothermic direction). This will favor the forward reaction, and thus, the equilibrium constant will increase.

Factors affecting equilibrium: Primarily involves alterations in pressure or volume, changes in concentration, and temperature modifications. Pressure and volume changes have significant impact on equilibrium.

The value of K (the equilibrium constant) for reaction depends only on temperature and is independent of the pressure or concentrations of reactants/products, presence of catalyst etc.

In an equilibrium process, a catalyst has no effect on the position of equilibrium. All it does is allow the reaction to reach equilibrium at a faster rate, but does not have any effect on the position of equilibrium. As always, the catalyst is not changed in the reaction.

The equilibrium constant is constant for a certain reaction at a specific temperature. It isn't affected by changes in pressure or concentration, or the presence of a catalyst. However, it is affected by temperature.

Temperature is the only factor that we learned affects K value. The direction of change in K value depends if the reaction is exothermic or endothermic. If the temperature increases, K will increase in an endothermic reaction and decrease in an exothermic reaction.

If the temperature of the system is increased, the equilibrium will shift away from the heat that may be stated in the equation. If the temperature of the system is decreased, the equilibrium will shift toward the heat that may be stated in the equation.