What is the equilibrium constant expression for each reactions?
1.) C2H2 + 3 O2 ---> 2 CO2 + 2 H2O
2.) 4 HI ---> 2 H2 + 2 I2
Keq = (products)^x/(reactants)^y
where x and y are the coefficients.
This is pretty fundamental. I'll be glad to check your answers if you will post.
The equilibrium constant expression for each reaction can be written as follows:
1.) For the reaction C2H2 + 3 O2 ---> 2 CO2 + 2 H2O, the equilibrium constant expression is:
Kc = ([CO2]^2 * [H2O]^2) / ([C2H2] * [O2]^3)
2.) For the reaction 4 HI ---> 2 H2 + 2 I2, the equilibrium constant expression is:
Kc = ([H2]^2 * [I2]^2) / ([HI]^4)
In these expressions, [CO2], [H2O], [C2H2], [O2], [H2], [I2], and [HI] represent the molar concentrations of each species at equilibrium. The exponents indicate the stoichiometric coefficients of each reactant or product in the balanced chemical equation.
To determine the equilibrium constant expressions for each reaction, we need to first identify the products and reactants in the balanced chemical equation.
1.) C2H2 + 3 O2 ---> 2 CO2 + 2 H2O
The reactants in this reaction are C2H2 and O2, and the products are CO2 and H2O. The equilibrium constant expression is given by the ratio of the concentrations of the products to the concentrations of the reactants, each raised to the power of their respective stoichiometric coefficients.
The equilibrium constant expression for this reaction is:
K = [CO2]^2 * [H2O]^2 / [C2H2] * [O2]^3, where [ ] represents the concentration of each species.
2.) 4 HI ---> 2 H2 + 2 I2
In this reaction, the reactant is HI and the products are H2 and I2. Following the same approach as before, we can write the equilibrium constant expression:
K = [H2]^2 * [I2]^2 / [HI]^4
So, the equilibrium constant expression for the second reaction is K = [H2]^2 * [I2]^2 / [HI]^4.