Question

Ammonia gas is synthesized according to the balanced equation below. N2 (g) + 3 H2 (g) → 2 NH3 (g) If 2.75 L N2 react with 7.75 L H2, what is the theoretical yield (in liters) of NH3?

Volumes of reactants and products are assumed to be measured at the same temperature and pressure.

(Should I convert the liters into grams to determine theoretical yield or should I leave them as they are?)

Answer 1

The balanced equation of the gaseous reaction given is

`N_2(g)+3H_2(g)->2NH_3(g)`

As per the reaction stochiometry we see that the gaseous ractants and products are in the following mole ratio `1:3:2` So ratio of their volume will also follow same ratio.

Hence to maintain that ratio the `2.75L" " N_2(g)` will react with `8.25L" " H_2(g)` to form theoretically `2*2.75L=5.50L" "NH_3(g)`
But the volume of `H_2(g)` will fall short then.So hydrogen given will be fully consumed and the yeild of `NH_3(g)` to be calculated on the consumption of of available `H_2(g) i.e.7.75L`

Si theoretical yeild of `NH_3(g)` will be `=2/3xx7.75L~~5.17L`