How many liters of hydrogen (N2) are needed to produce 100 liters of ammonia (NH3) by direct combination with?

Answer 1

use Lussac's Law.
so by Lussac's Law
N2+3H2---->2NH3
1 volume of N2+3 volumes of H2------->2 volumes of NH3
if 2 volumes of ammonia=100L(in this case)
1 volume of ammonia = 50L
hence 1 volume of Nitrogen=50L
and 3 volumes of Hydrogen=50*3L
=150L.
therefore we need 50L of nitrogen and 150L of hydrogen.

Answer 2

You need the balanced equation:
3H2 + N2 -> 2 NH3.

So for each 2 moles of ammonia, 3 moles of hydrogen are needed. From ideal gas law, V , the volume, is proportional to n, the number of moles. So we need 150 liters of H2 gas.

Answer 3

at standerd temprature and pressure each gass has its volume 22.414dm3.or 2.2414litters of its one mole.so if we need to prodece one mole of amonia we need 1.5 moles of hydrogen whom volume will be 2.2414*1.5=3.36liters. now we have to produce 100 liters of amonmia.so to produce one mole or 2.2414 liters of amonia we need 3.36 liters of hydrogen, then for 100liters of NH3, it will be 149.91 at STP liters of hydrogen are required. the volume of whole compound will be less at STP because now the molecule is bigger and bonding is between hetroatoms which is more stronger creating more compectness, decreasing repulsive forces.thats why when we add 149.91 liters of hydrogen and X liters of N we get 100 liters, less volume of amonia.