Jawaban:

To determine the rates of formation for ammonia and the rate of reaction for molecular nitrogen, we need to consider the stoichiometry of the balanced chemical equation:

N₂(g) + 3H₂(g) → 2NH₃(g)

(a) To find the rate at which ammonia is being formed, we can use the stoichiometric coefficients from the balanced equation. According to the equation, for every 3 moles of hydrogen reacted, 2 moles of ammonia are formed. Therefore, the rate at which ammonia is being formed is directly proportional to the rate of hydrogen consumption.

Given that the rate of hydrogen consumption is 0.074 M/s, we can set up a proportion to find the rate of ammonia formation:

(2 moles NH₃ / 3 moles H₂) = (rate of NH₃ formation / 0.074 M/s)

Simplifying the proportion:

rate of NH₃ formation = (2/3) * 0.074 M/s

rate of NH₃ formation ≈ 0.0493 M/s

Therefore, ammonia is being formed at a rate of approximately 0.0493 M/s.

(b) The rate at which molecular nitrogen is reacting can also be determined using the stoichiometric coefficients. According to the balanced equation, for every 1 mole of nitrogen reacted, 2 moles of ammonia are formed.

Using the same reasoning as before, the rate of nitrogen consumption is directly proportional to the rate of ammonia formation. Therefore, the rate at which molecular nitrogen is reacting is half the rate at which ammonia is being formed:

rate of N₂ reaction = (1/2) * rate of NH₃ formation

rate of N₂ reaction ≈ 0.0247 M/s

Therefore, molecular nitrogen is reacting at a rate of approximately 0.0247 M/s.