The mass of ammonia that would be produced is 312.5 g
First, we will write a balanced chemical equation for the reaction
The balanced chemical equation for the reaction is
3H₂(g) + N₂(g) → 2NH₃(g)
This means
3 moles of hydrogen gas reacts with 1 mole of nitrogen gas to produce 2 moles of ammonia.
First, we will determine the number of moles of each reactant present
For Hydrogen (H₂)
Mass = 83.6 g
Molar mass = 2.016 g/mol
Using the formula
![Number\ of\ moles = \frac{Mass}{Molar\ mass}](https://tex.z-dn.net/?f=Number%5C%20of%5C%20moles%20%3D%20%5Cfrac%7BMass%7D%7BMolar%5C%20mass%7D)
Number of moles of H₂ present = ![\frac{83.6}{2.016}](https://tex.z-dn.net/?f=%5Cfrac%7B83.6%7D%7B2.016%7D)
∴ Number of moles of H₂ present = 41.468254 moles
For Nitrogen (N₂)
Mass = 257 grams
Molar mass = 28.0134 g/mol
∴ Number of moles of N₂ present = ![\frac{257}{28.0134}](https://tex.z-dn.net/?f=%5Cfrac%7B257%7D%7B28.0134%7D)
Number of moles of N₂ present = 9.174181 moles
Since,
3 moles of hydrogen gas reacts with 1 mole of nitrogen gas to produce 2 moles of ammonia
Then,
27.522543 moles of hydrogen gas will react with the 9.174181 moles of nitrogen gas to produce 18.348362 moles of ammonia
∴ 18.348362 moles of ammonia will be produced during the reaction
Now, for the mass of ammonia that would be produced
From the formula
Mass = Number of moles × Molar mass
Molar mass of ammonia = 17.031 g/mol
Mass of ammonia that would be produced = 18.348362 × 17.031
Mass of ammonia that would be produced = 312.49095 g
Mass of ammonia that would be produced ≅ 312.5 g
Hence, the mass of ammonia that would be produced is 312.5 g
Learn more here: brainly.com/question/13902065