[" For the dissociation reaction "N_(2)O_(4)(g)rightleftharpoons2NO_(2)(g)," the degree of dissociation "(alpha)" in temst "],[K_(p)" and total equilibrium pressure "P" is : "]

For the dissociation reaction N_(2)O_(4) (g)hArr 2NO_(2)(g) , the degree of dissociation (alpha) interms of K_(p) and total equilibrium pressure P is:

For the dissociation reaction N_(2)O_($) (g)hArr 2NO_(2)(g) , the degree of dissociation (alpha) interms of K_(p) and total equilibrium pressure P is:

For the dissociation reaction N_(2)O_($) (g)hArr 2NO_(2)(g) , the degree of dissociation (alpha) interms of K_(p) and total equilibrium pressure P is:

For the reaction N_2O_4 (g) overset(rightarrow)(leftarrow)2NO_2 (g) at equilibrium the degree of dissociation (alpha) is 28% at temperature 318 K and total pressure 2 atm. Calculate the K_P and K_C for the reaction.

If in the reaction, N_(2)O_(4)(g)hArr2NO_(2)(g), alpha is the degree of dissociation of N_(2)O_(4) , then the number of moles at equilibrium will be

If in the reaction, N_(2)O_(4)(g)hArr2NO_(2)(g), alpha is the degree of dissociation of N_(2)O_(4) , then the number of moles at equilibrium will be

For the reaction N_(2)O_(4)(g)hArr2NO_(2)(g) , the degree of dissociation at equilibrium is 0.2 at 1 atm pressure. The equilibrium constant K_(p) will be

For the reaction N_(2)O_(4)(g)hArr2NO_(2)(g) , the degree of dissociation at equilibrium is 0.2 at 1 atm pressure. The equilibrium constant K_(p) will be

For the reaction, N_(2)O_(4)(g)hArr 2NO_(2)(g) the degree of dissociation at equilibrium is 0.l4 at a pressure of 1 atm. The value of K_(p) is

For the reaction, N_(2)O_(4)(g)hArr 2NO_(2)(g) the degree of dissociation at equilibrium is 0.14 at a pressure of 1 atm. The value of K_(p) is