Respuesta :
Answer:
Kc = 0.075
Explanation:
The dissociation (α) is the initial quantity that ionized divided by the total dissolved. So, let's calling x the ionized quantity, and M the initial one:
α = x/M
x = M*α
x = 0.354M
For the stoichiometry of the reaction (2:1:1), the concentration of H₂ and I₂ must be half of the acid. So the equilibrium table must be:
2HI(g) ⇄ H₂(g) + I₂(g)
M 0 0 Initial
-0.354M +0.177M +0.177M Reacts
0.646M 0.177M 0.177M Equilibrium
The equilibrium constant Kc is the multiplication of the products' concentrations (elevated by their coefficients) divided by the multiplication of the reactants' concentrations (elevated by their coefficients):
[tex]Kc = \frac{[H2]*[I2]}{[HI]^2}[/tex]
[tex]Kc = \frac{0.177M*0.177M}{(0.646M)^2}[/tex]
[tex]Kc = \frac{0.03133M^2}{0.41732M^2}[/tex]
Kc = 0.075
The equilibrium constant (Kc) is the proportion of the concentration of the products and the reactants. 0.075 is the Kc for the reaction at this temperature.
What is equilibrium constant?
The equilibrium constant (Kc) is the ratio of the concentration of the products of the reaction over the reactants raised to the powers of the stoichiometric coefficients.
The dissociation can be given as,
[tex]\begin{aligned}\alpha &= \rm \dfrac{x}{M}\\\\\rm x &= \rm M \times \alpha\\\\&= 0.354 \;\rm M\end{aligned}[/tex]
From the equilibrium table, the concentration of the initial reactant is -0.354 M and products are +0.177 M, while at the equilibrium reactant concentration is 0.646 and of products are 0.177 M.
The equilibrium constant (Kc) can be given as,
[tex]\begin{aligned}\rm K_{c} &= \rm \dfrac{[H_{2}][I_{2}]}{[HI]^{2}}\\\\&= \dfrac{0.177 \times 0.177}{(0.646)^{2}}\\\\&= 0.075 \end{aligned}[/tex]
Therefore, 0.075 is the equilibrium constant.
Learn more about the equilibrium constant here:
https://brainly.com/question/14018448
