`K_(p)` for equilibrium `N_(2)O_(4) hArr 2NO_(2)` is `0.25` at `15^(@)C`. If the system is allowed to expand `&` `N_(2)` is added at a constant pressure of 1 atm. What will be the degree when partial of `N_(2)` is 0.6 atm.

K_p for the reaction : N_2O_4(g) hArr 2NO_2(g) is 0.157 atm at 27^@C and 1 atm pressure . Calculate K_c for the reaction.

At 46^@C, K_p for the reaction N_2O_4(g) iff 2NO_2(g) is 0.66. Calculate the partial pressure of N_2O_4 and NO_2 at equilibrium and at a total pressure of 0.5 atm.

For the dissociation reaction N_(2)O_(4)(g)hArr2NO_(2)(g), the equilibrium constant K_(P) is 0.120 atm at 298 K and total pressure of system is 2 atm. Calculate the degree of dissociation of N_(2)O_(4) .

For the dissociation reaction N_(2)OhArr2NO_(2)(g), the equilibrium constant K_(P) is 0.120 atm at 298 K and total pressure of system is 2 atm. Calculate the degree of dissociation of N_(2)O_(4) .

In a container equilibrium N_(2)O_(4) (g)hArr2NO_(2) (g) is attained at 25^(@)C . The total equilibrium pressure in container is 380 torr. If equilibrium constant of above equilibrium is 0.667 atm, then degree of dissociation of N_(2)O_(4) at this temperature will be:

For the equilibrium N_(2)+3H_(2) hArr 2NH_(3) at 298K and 5 atm. Pressure, increasing pressure to 50 atm, will ( here K is the equilibrium constant )

In a mixture of N_(2) and O_(2) gases, the mole fraction of N_(2) is found to be 0.700. the total pressure of the mixture is 1.42atm. What is the partial pressure of O_(2) in the mixture?