Question

Consider the reaction represented by the (unbalanced) equation: N₂(g) + H₂(g) → NH₃(g). Determine the number of moles of NH₃(g) that can be produced from 0.63 mol N₂(g) reacts completely with H₂(g).

Answer 1

The number of moles of NH3(g) produced from 0.63 mol N2(g) is 1.26 moles, based on the stoichiometric ratio of 1 mol N2 to 2 moles NH3 in the balanced chemical equation.

Step-by-step explanation:

The question asks to determine the number of moles of NH3(g) that can be produced when 0.63 mol N2(g) reacts completely with H2(g). To solve this problem, we use the stoichiometry of the balanced chemical equation:

N2 (g) + 3H2 (g) → 2NH3 (g)

According to the balanced equation, 1 mole of N2 reacts with 3 moles of H2 to produce 2 moles of NH3. Therefore, the mole ratio of N2 to NH3 is 1:2. Using this ratio, we can find that 0.63 moles of N2 will produce 2 × 0.63 = 1.26 moles of NH3.