The degree of dissociation of `I_(2)` "mole"cule at `1000^(@)C` and under `1.0 atm` is `40%` by volume. If the dissociation is reduced to `20%` at the same temperature, the total equilibrium pressure on the gas will be:

the degree of dissociation of PCI_(5) at a certain temperature and under one atmosphere pressure is 0.2. Calculate the pressure at which it is half dissociated at the same temperature.

The degree of dissociation of N_(2)O_(4) into NO_(2) at 1 atm 40^(@)C is 0.310 . Calculate its K_(p) at 40^(@)C . Also report the degree of dissociation at 10 atm pressure at same temperature.

The degree of dissociation of PCl_(5) at 1 atm pressure is 0.2 . Calculate the pressure at which PCl_(5) is dissociated to 50% ?

The degree of dissociation of PCl_(5) at 1 atm pressure is 0.2 . Calculate the pressure at which PCl_(5) is dissociated to 50% ?

The degree of dissociation of PCl_(5) ata certain temperature and atmospheric pressure is 0*2 . Calculate the pressure at which it will be half (50 %) dissociated at the same temperature .

The equilibrium constant K_(p) for the thermal dissociation of PCl_(5) at 200^(@)C is 1.6 atm. The pressure (in atm) at which it is 50% dissociated at that temperature is

Find the percentage dissociation of ammonia into N_(2) "and' H_(2) if the dissociation is carried out at constant pressure and the volume at equilibrium is 20% greater than initial volume. (Initially. Equal moles of NH_(3) "and" N_(2) are present with no hydrogen)