5 moles of `SO_2` and 5 moles of `O_2` are mixed to produce `SO_3`. At equilibrium it was found that 60% of `SO_2` is used up. If the pressure of the equilibrium mixture is 1 atmosphere. The partial pressure of `O_2` is

5 moles of SO_(2) and 5 moles of O_(2) are allowed to react .At equilibrium , it was foumnd that 60% of SO_(2) is used up .If the pressure of the equilibrium mixture is one aatmosphere, the parital pressure of O_(2) is :

A gaseous mixture was prepared by taking equal moles of CO and N_2 . If the total pressure of the mixture was found 1 atmosphere, the partial pressure of the nitrogen (N_2) in the mixture is

5 moles of SO_(2) and 5 moles of O_(2) are allowed to react to form SO_(3) in a closed vessel. At the equilibrium stage 60% of SO_(2) is used up. The total number of moles of SO_(2), O_(2) and SO_(3) in the vessel now is

5 mole of X are mixed with 3 moles of Y. At equilibrium for the reaction, X + Y rarr Z 2 moles of Z are formed. The equilibrium constant for the reaction will be

4 moles each of SO_(2) "and" O_(2) gases are allowed to react to form SO_(3) in a closed vessel. At equilibrium 25% of O_(2) is used up. The total number of moles of all the gases at equilibrium is

1 mole of sample of O_2 and 3 mole sample of H_2 are mixed isothermally in a 125.3 litre container at 125^@C the total pressure of gaseous mixture will be

a' moles of PCI_(5) , undergoes, thermal dissociation as: PCI(5)hArrPCI_(3)+CI_(2) , the mole of PCI_(3) equilibrium is 0.25 and the total pressure is 2.0 atmosphere. The partial pressure of CI_(2) at equilibrium is:

Starting with one moles of O_(2) and two moles of SO_(2) , the equilibrium for the formation of SO_(3) was established at a certain temperature. If V is the volume of the vessel and 2 x is the number of moles of SO_(3) present, the equilibrium cosntant will be

For the reaction 2SO_2 + O_2 to 2SO_3 , the unit of equilibrium constant is :