Respuesta :
Answer : The value of equilibrium constant (Kc) is, 0.0154
Explanation :
The given chemical reaction is:
[tex]SO_2Cl_2(g)\rightarrow SO_2(g)+Cl_2(g)[/tex]
Initial conc. [tex]2.4\times 10^{-2}[/tex] 0 0
At eqm. [tex](2.4\times 10^{-2}-x)[/tex] x x
As we are given:
Concentration of [tex]Cl_2[/tex] at equilibrium = [tex]1.3\times 10^{-2}M[/tex]
That means,
[tex]x=1.3\times 10^{-2}M[/tex]
The expression for equilibrium constant is:
[tex]K_c=\frac{[SO_2][Cl_2]}{[SO_2Cl_2]}[/tex]
Now put all the given values in this expression, we get:
[tex]K_c=\frac{(x)\times (x)}{2.4\times 10^{-2}-x}[/tex]
[tex]K_c=\frac{(1.3\times 10^{-2})\times (1.3\times 10^{-2})}{2.4\times 10^{-2}-1.3\times 10^{-2}}[/tex]
[tex]K_c=0.0154[/tex]
Thus, the value of equilibrium constant (Kc) is, 0.0154
