## Why is equilibrium constant not affected by concentration?

As detailed in the above section, the position of equilibrium for a given reaction does not depend on the starting concentrations and so the value of the equilibrium constant is truly constant. This is because equilibrium is defined as a condition resulting from the rates of forward and reverse reactions being equal.

## Why is equilibrium constant dependent on temperature?

The value of the equilibrium constant depends on temperature for two reasons. There is a factor of the temperature in the relationship between the standard free energy and K. For exothermic reactions, as \(T\) increases \(K\) decreases (more reactants at equilibrium than at the previous temperature).

What does a high equilibrium constant mean?

If K is a large number, it means that the equilibrium concentration of the products is large. In this case, the reaction as written will proceed to the right (resulting in an increase in the concentration of products) If K is a small number, it means that the equilibrium concentration of the reactants is large.

Which is the correct formula for the equilibrium constant KC?

The ratio of the rate constant of forward reaction to the rate constant of backward reaction should be a constant and is called an equilibrium constant (K equ ). where Kc, indicates the equilibrium constant measured in moles per litre. For reactions involving gases: The equilibrium constant formula, in terms of partial pressure will be:

### Which is the equilibrium constant for the reverse reaction?

K’ is the constant for the reverse reaction and K is that of the forward reaction. Example: What is the value of the equilibrium constant for the reaction 2 NO2(g) N2O4(g) at 100oC? N2O4(g) 2 NO2(g) Kc= 0.212 @ 100oC? The desired reaction is the reverse of the reaction for which the Kcis known.

### How is the equilibrium expression of a balanced equation calculated?

The equilibrium expression is the reciprocal of that given. If the coefficients in a balanced equation are multiplied by a factor, n, the equilibrium expression is raised to the n th power. K’ is the constant for the reaction multiplied by n and K is the constant of the original reaction.

Why does the magnitude of the equilibrium constant depend on the form?

Because equilibrium can be approached from either direction in a chemical reaction, the equilibrium constant expression and thus the magnitude of the equilibrium constant depend on the form in which the chemical reaction is written. For example, if we write the reaction described in Equation 15.2.4 in reverse, we obtain the following: