Answer:
Hydrogen is the excess reactant
Nitrogen is the limiting reactant
151.6g is theoretical yield
Explanation:
The reaction of N₂ with H₂ to produce NH₃ is:
N₂ + 3H₂ → 2NH₃
To find theoretical yield we need to determine limiting reactant with the moles of each gas as follows:
Nitrogen -Molar mass: 28g/mol-
125.0g * (1mol / 28g) = 4.46 moles
Hydrogen -Molar mass: 2g/mol-
125.0g * (1mol / 2g) = 62.5 moles of hydrogen
For a complete reaction of 4.46 moles of N2 there are needed:
4.46 moles N2 * (3moles H2 / 1mol N2) = 13.38 moles of hydrogen
As there are 62.5 moles of hydrogen:
<h3>Hydrogen is the excess reactant</h3><h3>Nitrogen is the limiting reactant</h3><h3 />
With nitrogen, the limiting reactant, we determine theoretical moles (Assuming 100% of the reaction occurs) and theoretical yield (In mass):
4.46 moles N2 * (2moles NH3 / 1mol N2) = 8.92 moles of ammonia
As molar mass of ammonia is 17g/mol:
8.92 moles of ammonia * (17g/mol) =
<h3>151.6g is theoretical yield</h3>
