Understanding the Equilibrium Constant Expression
Posted: Fri Apr 05, 2024 12:43 am
Hello fellow chemists,
I've been studying chemical equilibrium and came across a reaction where the equilibrium constant expression seems a bit complex. The reaction is as follows:
$$\text{aA} + \text{bB} \rightleftharpoons \text{cC} + \text{dD}$$
Given that the stoichiometric coefficients are integers, how would you derive the expression for the equilibrium constant ( K )? Additionally, how does the change in concentration of one of the reactants affect the equilibrium position?
I've been studying chemical equilibrium and came across a reaction where the equilibrium constant expression seems a bit complex. The reaction is as follows:
$$\text{aA} + \text{bB} \rightleftharpoons \text{cC} + \text{dD}$$
Given that the stoichiometric coefficients are integers, how would you derive the expression for the equilibrium constant ( K )? Additionally, how does the change in concentration of one of the reactants affect the equilibrium position?