We need (i) the stoichiometric equation, and (ii) the equivalent mass of dihydrogen. Explanation: 1 2 N 2 ( g ) + 3 2 H 2 ( g ) → N H 3 ( g ) 11.27
g of ammonia represents 11.27 ⋅ g 17.03 ⋅ g ⋅ m o l − 1
=
? ?
m o l . Whatever this molar quantity is, it is clear from the stoichiometry of the reaction that 3/2 equiv of dihydrogen gas were required. How much dinitrogen gas was required?
