If `340 g` of a mixture of `N_(2)` and `H_(2)` in the correct ratio gas a `20%` yield of `NH_(3)`. The mass produced would be:

If 340 g of a mixture of N_2 and H_2 in the correct ratio has a 20% yield of NH_3 . The mass produced would be

If 340 g of mixture N_2 and H_2 in the correct raito gave a 20% yield of NH_3 . The mass produced would be:

90 gm mixture of H_(2) and O_(2) is taken In stoichiometric ratio and gives H_(2)O with 50% yield. The produced mass of H_(2)O (in gm) is :

A gaseous mixture of H_(2) and NH_(3) gas contains 68 mass % of NH_(3) . The vapour density of the mixture is-

A gaseous mixture of H_(2) and NH_(3) gas contains 68 mass % of NH_(3) . The vapour density of the mixture is-

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) .

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) .

If 1:3 (molar ratio) mixture of N_2 and H_2 yields 20% (by volume) of NH_3 at 30 atm , then the moles of N_2 converted into the product at equilibrium will be