Gaseous `N_2O_4` dissociates into gaseous `NO_2` according to the reaction `N_2O_4(g) hArr 2NO_2(g)` .At 300 K and 1 atm pressure, the degree of dissociation of `N_2O_4` is 0.2 If one mole of `N_2O_4` gas is contained in a vessel, then the density of the equilibrium mixture is :

Gaseous N_(2)O_(4) dissociates into gaseous NO_(2) according to the reaction : [N_(2)O_(4)(g)hArr2NO_(2)(g)] At 300 K and 1 atm pressure, the degree of dissociation of N_(2)O_(4) is 0.2. If one mole of N_(2)O_(4) gas is contained in a vessel, then the density of the equilibrium mixture is :

For the reaction N_(2)O_(4)hArr 2NO_(2(g)), the degree of dissociation of N_(2)O_(4) is 0.2 at 1 atm. Then the K_(p) of 2NO_(2)hArr N_(2)O_(4) is

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_2O_4 harr 2NO_(2(g)) , the degree of dissociation at equilibrium is 0.2 at 1 atm. Then K_p will be

For the reaction , N_2O_4(g)hArr2NO_2(g) the degree of dissociation at equilibrium is 0.4 at a pressure of 1 atm. The value of K_p is

K_p for the reaction N_2O_4(g) leftrightarrow 2NO_2(g) at 750K is 640torr. Calculate the percentage of dissociation of N_2O_4 at equilibrium pressure of 160torr.