Using the data given below, calculate the value of equilibrium constant for the reaction. `underset("Acetylene")(3HC-=CH(g)) hArr underset("Benzene")(C_(6)H_(6)(g))` at 298 K , assuming ideal gas behaviour. `Delta_(f)G^(@) ` for `HC-= CH(g) = 2.09 xx 10^(5) J mol^(-1), Delta_(f)G^(@) ` for`C_(6)H_(6)(g) =1.24xx 10^(5) J mol^(-1)` `R = 8.314 J K^(-1) mol^(-1)` Based on your calculated value, comment whether this process can be recommended as a practical method for making benzene.

Using the data given below, calculate the value of equilibrium constan

1.	Using the data given below, calculate the value of equilibrium constant for the reaction. `underset("Acetylene")(3HC-=CH(g)) hArr underset("Benzene")(C_(6)H_(6)(g))` at 298 K , assuming ideal gas behaviour. `Delta_(f)G^(@) ` for `HC-= CH(g) = 2.09 xx 10^(5) J mol^(-1), Delta_(f)G^(@) ` for`C_(6)H_(6)(g) =1.24xx 10^(5) J mol^(-1)` `R = 8.314 J K^(-1) mol^(-1)` Based on your calculated value, comment whether this process can be recommended as a practical method for making benzene.
Answer» Correct Answer - `K = 1.43 xx 10^(88) ,` Yes `Delta_(r) G^(@) =Delta_(f)G^(@) (C_(6)H_(6)) - 3 Delta_(f)G^(@) (HC -= CH) = 1.24 xx 10^(5) - 3 ( 2.9 xx 10^(5)) J = - 5.03 xx 10^(5)J` `Delta_(r)G^(@) = - 2.303 RT log K `. Calculate K `Delta _(r)G^(@) ` is negative and K is very high . Hence, the process can occur easily.

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