Ammonia gas at 76 cm Hg pressure was connected to a manometer. After sparking in the flask, ammonia is partially dissociated as follows :
`2NH_(3) (g) hArr N_(2) (g) + 3H_(2) (g)`
the level in the mercury column of the manometer was found to show the difference of 18 cm. What is the partial pressure of `H_(2) (g)` at equilibrium ?

A manometer attached to a flask contains with ammonia gas have no difference in mercury level initially as shown in diagram. After sparking into the flask, ammonia is partially dissociated as 2NH_(3)" (g)"rarr N_(2)" (g)"+3H_(2)" (g)" now it have difference of 6 cm in mercury level in two columns, what is partial pressure of H_(2)" (g)" at equilibrium?

A manometer attached to a flask contains with ammonia gas have no difference in mercury level initially as shown in diagram. After sparking into the flask, ammonia is partially dissociated as 2NH_(3)" (g)"rarr N_(2)" (g)"+3H_(2)" (g)" now it have difference of 6 cm in mercury level in two columns, what is partial pressure of H_(2)" (g)" at equilibrium?

A sample of pure NO_2 gas heated to 1000 K decomposes : 2NO_2(g) hArr 2NO(g)+O_(2)(g) The equilibrium constant K_P is 100 atm. Analysis shows that the partial pressure of O_2 is 0.25 atm. At equilibrium.The partial pressure of NO_2 at equilibrium is:

Two moles of ammonia gas are introduced into a previously evacuated 1 L flask in which it partially dissociates at high temperature as : 2NH_(3)(g)hArr N_(2)(g)+3H_(2)(g) At equilibrium 1.0 mole of NH_(3)(g) is found. What is K_(c ) ?

N_(2)(g)+3H_(2)(g)hArr2NH_(3)(g) For the reaction intially the mole ratio was 1:3 of N_(2):H_(2) .At equilibrium 50% of each has reacted .If the equilibrium pressure is P, the parial pressure of NH_(3) at equilibrium is :

N_(2)(g)+3H_(2)(g)hArr2NH_(3)(g) For the reaction intially the mole ratio was 1:3 of N_(2):H_(2) .At equilibrium 50% of each has reacted .If the equilibrium pressure is P, the parial pressure of NH_(3) at equilibrium is :

N_(2)(g)+3H_(2)(g)hArr2NH_(3)(g) For the reaction intially the mole ratio was 1:3 of N_(2):H_(2) .At equilibrium 50% of each has reacted .If the equilibrium pressure is P, the parial pressure of NH_(3) at equilibrium is :

N_(2(g)) + 3H_(2(g)) hArr 2NH_(3(g)) for the reaction initially the mole ratio was 1: 3 of N_(2). H_(2) . At equilibrium 50% of each has reacted. If the equilibrium pressure is p, the partial pressure of NH_(3) at equilibrium is

N_(2(g)) + 3H_(2(g)) hArr 2NH_(3(g)) for the reaction initially the mole ratio was 1: 3 of N_(2). H_(2) . At equilibrium 50% of each has reacted. If the equilibrium pressure is p, the partial pressure of NH_(3) at equilibrium is