To determine the mass of hydrogen that will react with 84g of N2, we need to use stoichiometry and balanced chemical equation for the reaction between nitrogen (N2) and hydrogen (H2).
The balanced chemical equation for this reaction is:
N2 + 3H2 → 2NH3
This means that one mole of N2 reacts with three moles of H2 to produce two moles NH3.
To find out how many moles of N₂ are present in 84 g, we can use its molar mass which is about 28 g/mol.
Number of Moles = Given Mass / Molar Mass
= 84 g /28 g/mol
= 3 mol
From the balanced chemical equation above, we know that it takes three moles of H₂ to react with one mole N₂. Therefore,
1 mol N₂ : 3 mol H₂
Using these ratios, we can calculate the number of moles needed for Hydrogen.
Moles H₁= Ratio * given amount
= (3/1)* Number_of_Moles_Nitrogen
=(3/1)* (3mol)
=9mol
Now that you have calculated how many moles are needed based on stoichiometry calculation, you can now calculate the mass using :
Mass= Number Of Moles * Molar Mass
=9mol* (about) 2g/mol
≈18 g
Therefore, approximately **18 grams** of hydrogen will react with **84 grams**of Nitrogen.