The ratio of the rate of diffusion of a sample of `N_(2)O_(4)` partially dissociated in to `NO_(2)` to pure hydrogen was found to be `1:5` . Calculate the degree of dissociation of `N_(2)O_(4)`.
At 60^(@) and 1 atm, N_(2)O_(4) is 50% dissociated into NO_(2) then K_(p) is
The vapour density of N_(2)O_(4) at a certain temperature is 30 . Calculate the percentage dissociation of N_(2)O_(4) this temperature.
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) .
During thermal dissociation, the observed vapour density of N_(2)O_(4)(g) is 26.0. The extent of dissociation of N_(2)O_(4) is:
The N_(2)O_(4)//NO_(2(g)) equilibrium is endothermic as shown below: underset(Colourl es)(N_(2)O_(4(g)))hArrunderset(Dark brown)(2NO_(2(g))) , ( DeltaH=+ve ) The equilibrium is attained in a container having movable piston by taking 1 mol e of N_(2)O_(4(g)) at 50^(@)C and 1 atm pressure. At equilibrium, relative molecular mass of the mixture is 65.7 . The degree of dissociation of N_(2)O_(4) at equilibrium is:
In a container initially only N_(2)O_(4) is present and no difference in height of Hg-column of two limbs : If due to dissociation of N_(2)O_(4) at constant temperature the difference in the column of mercury becomes 7.6 cm then calculate % dissociation of N_(2)O_(4).[N_(2)O_(4) rarr 2NO_(2)]
