The Haber Process is a method for the production of ammonia, an important chemical intermediate. The reaction for this process is N₂ + 3H₂ → 2NH₃
According to the mole interpretation, how many grams of NH₃ could be produced by the complete reaction of 2.80 grams of N₂ and excess H₂?

Question

Quizplus · Accepted Answer

First, calculate the molar mass of $N_2$ (28.02 g/mol) and $NH_3$ (17.03 g/mol). Given 2.80 g of $N_2$, we find the moles of $N_2$ (2.80 g / 28.02 g/mol = 0.1 mol). The stoichiometry of the reaction shows that 1 mole of $N_2$ produces 2 moles of $NH_3$, so 0.1 mol of $N_2$ will produce 0.2 mol of $NH_3$. Finally, convert moles of $NH_3$ to grams (0.2 mol * 17.03 g/mol = 3.406 g), which rounds to 3.40 g.

The Haber Process Is a Method for the Production of Ammonia