determine the experssion of equilbirum constant for h2+12=2Hi
The balanced equation for the reaction is:
H2(g) + I2(g) → 2HI(g)
The equilibrium constant expression, Kc, 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 coefficients in the balanced equation.
Kc = [HI]^2 / [H2][I2]
Where [HI], [H2], and [I2] represent the equilibrium concentrations of HI, H2, and I2, respectively.
The balanced chemical equation for the reaction you provided is:
H2 + I2 ⇌ 2 HI
The expression for the equilibrium constant (Kc) is determined by the concentrations of the reactants and products at equilibrium. In this case, it can be written as:
Kc = [HI]^2 / [H2] * [I2]
Where [HI], [H2], and [I2] represent the concentrations of HI, H2, and I2 respectively. Please note that the square brackets denote concentrations.
If the reaction is given in terms of partial pressures, the expression for the equilibrium constant (Kp) can be written as:
Kp = (p(HI))^2 / (p(H2) * p(I2))
Where p(HI), p(H2), and p(I2) represent the partial pressures of HI, H2, and I2 respectively.
To determine the expression for the equilibrium constant of the given reaction:
H2 + I2 ⇌ 2HI
The equilibrium constant (K) for this reaction can be expressed using the concentrations of the species involved in the reaction.
The general expression for the equilibrium constant is:
K = [C]^c [D]^d / [A]^a [B]^b
Where [A], [B], [C], and [D] represent the concentrations of the reactants and products, and a, b, c, and d represent their stoichiometric coefficients, respectively.
In our given reaction:
H2 + I2 ⇌ 2HI
The stoichiometric coefficients are 1 for H2, 1 for I2, and 2 for HI. Therefore, the expression for the equilibrium constant becomes:
K = [HI]^2 / [H2] [I2]
In this expression, [H2], [I2], and [HI] represent the concentrations of H2, I2, and HI at equilibrium, respectively.
Please note that the square brackets denote concentration in molarity (mol/L).