Step-by-step explanation:
We have to find the volume of H₂ that is needed to react with 5.2 L of N₂ at STP.
One mol of any gas at STP occupies 22.4 L. We can use that relationship to find the number of moles of N₂ that are present in 5.2 L of it.
1 mol of N₂ = 22.4 L
moles of N₂ = 5.2 L * 1 mol /(22.4 L)
moles of N₂ = 0.232 mol
N₂ (g) + 3 H₂ (g) ----> 2 NH₃ (g)
According to the coefficients of the reaction 1 mol of N₂ will react with 3 moles of H₂. So, the molar ratio between N₂ and H₂ is 1 to 3. We can use that relationship to find the number of moles of H₂ that will be needed to completely react with 0.232 moles of N₂.
1 mol of N₂ = 3 moles of H₂
moles of H₂ = 0.232 moles of N₂ * 3 moles of H₂/(1 mol of N₂)
moles of H₂ = 0.696 moles
And finally we can convert back the moles into liters.
1 mol of H₂ = 22.4 L (at STP)
volume of H₂ = 0.696 moles * 22.4 L/(1 mol)
volume of H₂ = 15.6 L
Answer: 15.6 L of hydrogen gas are needed to completly react with 5.2 L of nitrogen gas.