Dinitrogen and dihydrogen react with each other to produce ammonia according to the following chemical equation : N_(2(g))+H_(2(g)) rarr 2NH_(3(g)) (i) Calculate the mass of ammonia produced if 2.00xx10^(3)g dinitrogen reacts with 1.00xx10^(3) g of dihydrogen. (ii) Will any of the two reactants remain unreacted ? (iii) If yes, which one andwhat would be its mass ?

Dinitrogen and dihydrogen react with each other to produce ammonia acc

1.	Dinitrogen and dihydrogen react with each other to produce ammonia according to the following chemical equation : N_(2(g))+H_(2(g)) rarr 2NH_(3(g)) (i) Calculate the mass of ammonia produced if 2.00xx10^(3)g dinitrogen reacts with 1.00xx10^(3) g of dihydrogen. (ii) Will any of the two reactants remain unreacted ? (iii) If yes, which one andwhat would be its mass ?
Answer» Solution :`{:(N_(2(g)),+,3H_(2),rarr,2NH_(3(g)),),(1" mol",,3 " mol",,2 " mol",),(28 gm,,6 gm,,34 gm,):}` 28 gm `N_(2)` react with 6 gm `H_(2)` `:. 2000 gm N_(2) rarr (?)` `= (2000 xx 6)/(28) = 428.57 g H_(2)` (i) Here, `N_(2)` is LIMITING reagent So, created volume of ammonia. From 28 gm `N_(2)`, 34 gm `NH_(3)` create. `:.2000 gm N_(2) rarr (?)` `= (2000xx34)/(28) = 2428.57 g NH_(3)` (ii) Here, `N_(2)` is limiting reagent So, `H_(2)` become excess. (unreacted) (III) REMAINING mass of `H_(2)` gas `= 1000-428.57` `= 571.43g`