In a mixture of `N_(2)` and `H_(2)` in the ratio `1:3` at `30 atm` and `300^(@)C`, the `%` of `NH_(3)` at equilibrium is `17.8`. Calculate `K_(p)` for `N_(2)+3H_(2)hArr2NH_(3)`.

In a mixture of N_(2) and H_(2) in the ratio 1:3 at 30 atm and 300^(@)C , the % of NH_(3) at equilibrium is 17.8 . Calculate K_(p) for N_(2)+3H_(2) hArr 2NH_(3) .

In a mixture of N_(2) and H_(2) in the ratio 1:3 at 30 atm and 300^(@)C , the % of NH_(3) at equilibrium is 17.8 . Calculate K_(p) for N_(2)+3H_(2) hArr 2NH_(3) .

2 mol of N_(2) is mixed with 6 mol of H_(2) in a closed vessel of 1L capacity. If 50% of N_(2) is converted into NH_(3) at equilibrium, the value of K_(C ) for the reaction N_(2)(g0+3H_(2)(g)hArr 2NH_(3)(g) is

2 mol of N_(2) is mixed with 6 mol of H_(2) in a closed vessel of one litre capacity. If 50% N_(2) is converted into NH_(3) at equilibrium, the value of K_(c) for the reaction N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g)

2 mol of N_(2) is mixed with 6 mol of H_(2) in a closed vessel of one litre capacity. If 50% N_(2) is converted into NH_(3) at equilibrium, the value of K_(c) for the reaction N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g)

A mixture of N_2 and H_2 in the molar ratio of 1:3 reacts to give NH_3 developing an equilibrium pressure of 50 atm and 650 ^@C . NH_3 present at equilibrium at equilibrium is 25% by weight, calculate K_p for N_2(g) +3H_3(g) hArr 2NH_3(g)

A mixture of N_2 and H_2 in the molar ratio of 1:3 reacts to give NH_3 developing an equilibrium pressure of 50 atm and 650 ^@C . NH_3 present at equilibrium at equilibrium is 25% by weight, calculate K_p for N_2(g) +3H_3(g) hArr 2NH_3(g)