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

Explanation

(i) `"1 mole of N"_(2)," i.e., 28 g react with 3 moles of H"_(2)," i.e., 6 g of H"_(2)`
`therefore " 2000g of N"_(2)" will react with "H_(2)=(6)/(28)xx200g=428.6g." Thus, "N_(2)" is the limiting reagent while H"_(2) " is the excess reagent."`
2 moles of `N_(2)`, i.e., 28 g of `N_(2)` produce `NH_(3)` = 2 moles = 34 g
`therefore " 2000 g of N"_(2)" will produce NH"_(3)=(34)/(28)xx2000g=22428.57g`
(ii) `H_(2)` will remain unreacted.
(iii) Mass left unreacted `=1000g-428.6g=571.4g`