A gaseous mixture contain `2` moles of `N_(2)(g)` and `3` moles of `O_(2)(g)` then mole fraction of `O_(2)(g)` will be
`0.5`
`0.2`
`0.4`
`0.6`

At 127°C and l atm pressure, a mixture of a gas contains 0.3 mole of N_(2) , 0.2 mole of O_(2) The volume of the mixture is

The vapour density of a mixture containing N_(2) (g) and O_(2) (g) is 14.4. The percentage of N_(2) in the mixture is :

A gaseous mixture contains CO_(2) (g) and N_(2)O (g) in a 2 : 5 ratio by mass. The ratio of the number of molecules of CO_(2) (g) and N_(2)O is

0.5 mole of P_(4)O_(10) contains

The vapour density of a mixture containing NO_2 and N_2 O_4 is 27.6 . The mole fraction of N_2 O_4 in the mixture is :

The number of mole of N_(2)O_(4) in 276 g N_(2)O_(4) are …..

A gaseous mixture contains 1 g of H_(2) , 4 g of He , 7 g of N_(2) and 8 g of O_(2) . The gas having the highest partial pressure is :-

Average molecular weight of a gaseous mixture which contains 80% by mole N_(2) & rest O_(2) gas is-

For the reaction CO_2(g) +H_2 hArr CO(g) +H_2O(g) The K_c for the reaction is 0.11 if the reaction was started with 0.45 moles of CO_2 and 0.45 moles of H_2 at 700k ,the concentration of CO_2 when 0.34 mole of CO_2 and 0.34 mole of H_2 are added when the first equilibrium is attained is

A mixture of 3 moles of SO_(2) , 4 moles of NO_(2) , 1 mole of SO_(3) and 4 moles of NO is placed in a 2.0L vessel. SO_(2)(g)+NO_(2)(g) iff SO_(3)(g)+NO(g) . At equilibrium, the vessel is found to contain 1 mole of SO_(2) . Calculate the value of K_(C) .