How many grams of hydrogen are necessary to react completely with 50.0 g of nitrogen in the above reaction?
In the given reaction 3 moles of hydrogen react with 1 mole of nitrogen.
First, we need to find the molar mass of both hydrogen and nitrogen:
Hydrogen (H2):
Molar mass = 2.016 g/mol
Nitrogen (N2):
Molar mass = 28.02 g/mol
Now, calculate the moles of nitrogen present in 50.0 g of nitrogen:
moles of N2 = mass / molar mass
moles of N2 = 50.0 g / 28.02 g/mol
moles of N2 = 1.783 mol
According to the reaction, 1 mole of nitrogen reacts with 3 moles of hydrogen.
Therefore, moles of H2 needed = 1.783 mol x 3 = 5.35 mol
Now, calculate the mass of hydrogen needed:
mass of H2 = moles x molar mass
mass of H2 = 5.35 mol x 2.016 g/mol
mass of H2 = 10.78 g
Therefore, 10.78 grams of hydrogen is necessary to react completely with 50.0 g of nitrogen.