Respuesta :
Answer: Thus value of the equilibrium constant is 1.86
Explanation:
Moles of [tex]CH_2Cl_2[/tex] at equilibrium= 0.203 mole
Moles of [tex]CH_4[/tex] at equilibrium = 0.323 mole
Moles of [tex]CCl_4[/tex] at equilibrium = 0.240mole
Volume of solution = 15.2 L
Equilibrium concentration of [tex]CH_2Cl_2[/tex] = [tex]\frac{moles}{Volume}=\frac{0.203}{15.2}=0.0134M[/tex]
Equilibrium concentration of [tex]CH4[/tex] = [tex]\frac{moles}{Volume}=\frac{0.323}{15.2}=0.0212M[/tex]
Equilibrium concentration of [tex]CCl_4[/tex] = [tex]\frac{moles}{Volume}=\frac{0.240}{15.2}=0.0158M[/tex]
The given balanced equilibrium reaction is,
[tex]2CH_2Cl_2(g)\rightleftharpoons CH_4(g)+CCl_4(g)[/tex]
The expression for equilibrium constant for this reaction will be,
[tex]K_c=\frac{[CH_4]\times [CCl_4]}{[CH_2Cl_2]^2}[/tex]
Now put all the given values in this expression, we get :
[tex]K_c=\frac{0.0212\times 0.0158}{(0.0134)^2}[/tex]
[tex]K_c=1.86[/tex]
Thus value of the equilibrium constant is 1.86
