A Clear Explanation on the Characteristics of Equilibrium Constant

What is equilibrium constant: The equilibrium constant of a chemical reaction is the value of the reaction quotient at chemical equilibrium, and if its composition does not show a measurable tendency to change further, then the dynamic chemical system is approaching after sufficient time has passed. Under a given set of reaction conditions, the equilibrium constant is independent of the initial analytical concentration of reactants and product species in the mixture. Therefore, given the initial configuration of the system, known equilibrium constant values ​​can be used to determine the configuration of the system in equilibrium. However, reaction parameters such as temperature, solvent, and ionic strength can all affect the value of the equilibrium constant. Knowledge of the equilibrium constant is essential for understanding many chemical systems, as well as biochemical processes such as haemoglobin-mediated oxygen transport in the blood and acid-base homeostasis in the human body. Stability constants, formation constants, coupling constants, coupling constants, and dissociation constants are all types of equilibrium constants.

Characteristics of Equilibrium: The important properties of the equilibrium constant are described below. 

• The equilibrium constant has a specific value for a reaction at a specific temperature. 
• The value of the equilibrium constant is independent of the initial concentration of the reactants. 
• The value of the equilibrium constant indicates how much the reaction proceeds in the forward or reverse direction. If the value of K is large, the equilibrium concentration of the component on the right side of the reaction will be greater than the equilibrium concentration of the component on the left side of the reaction. Therefore, the reaction proceeds larger and vice versa. 
• The equilibrium constant is independent of the presence of the catalyst. This is because the catalyst affects the rates of both forward and reverse reactions equally. 
• In a reversible reaction, the constant of the forward reaction is that the opposite of the constant of the reverse reaction. 
• K forward reaction> = one / K reverse reaction> 
• The constant depends on the given temperature as follows. 
• Log K2 / K1 = ∆H / a pair of.303R [1 / T1 – one / T2 

 Here, K1 and K2 square measure the equilibrium constants at the temperatures T1 and T2, severally, and ΔH is the heat content amendment of the reaction. ∆H is assumed to be temperature freelance.

How to calculate the equilibrium constant: In the case of the equilibrium AA + BB ≧ CC + DD, the equilibrium constant can be found using the formula K = [C] C [D] D / [A] A [A] A [B] B. Here, k is a constant. The concentration of all the products is in the counter and the concentration of all reactants is in the denominator. Each component is raised to the power of that particular coefficient. The equilibrium constant is equal to the velocity constant of the forward reaction divided by the reverse reaction rate constant. 

 This relationship, equilibrium constant is known as a mass effect law. First, the law states that the chemical reaction rate is directly proportional to the concentration of the reactant. Second, and more importantly for us now, we also state that the concentration ratio of reactant to product is constant for the equilibrium reaction. This constant is known as the equilibrium constant K. 

 Also, the relationship of K = [C] c [D] d / [A] a [B] b is directly equivalent to K = kforward / kreverse, where kforward is the forward reaction and the rate constant of kreverse. Is the rate constant of the reverse reaction? 

Rate forward = kforward x [A] a [B] b 

 & Rate reverse = kreverse x [C] c [D] d 

 Therefore, kforward / kreverse = [C] c [D] d / [A] a [B] b = K … 

 This equation also explains why K indicates the magnitude of the reaction. If K> 1, the numerator represented by the product density will be large. If k <1, the denominator represented by the concentration of the reactant is larger.

Equilibrium constant formula: Kequ = kf / kb = [C] c [D] d / [A] a [B] b = Kc 

 where Kc is the equilibrium constant measured by the number of moles per litre. 

 For reaction with gas: The formula of the equilibrium constant related to partial pressure is as follows. 

Kequ = kf / kb = [[pC] c [pD] d] / [[pA] a [pB] b] = Kp 

 where Kp is the equation for the equilibrium constant for partial pressure. The larger the 

 Kc / Kp value, the more product formation and the higher the conversion rate. 

 The lower the Kc / Kp value, the less product formation and the lower the conversion rate. 

 Average Kc / Kp values ​​indicate optimal product formation

Units of Equilibrium Constant: The equilibrium constant is the ratio of the increase in concentration to the stoichiometric coefficient. Therefore, the unit of the equilibrium constant = [molL-1] Δn. 

 where ∆n = sum of stoichiometric coefficients of the product – sum of stoichiometric coefficients of the reactants.

CONCLUSION: The equilibrium constant defined by the volume fraction), the copolymer is between the components (χab, χ = 0) only if KABKBA> 1 (heterodox dominance, specific tendency towards alternate copolymers). It can be formed within the system without interaction.