Question

The reaction for the haber process, the industrial production of ammonia, is

N₂(g) + 3H₂(g) --> 2NH₃(g)


assume that under certain laboratory conditions ammonia is produced at the rate of 6.29 x 10⁻⁵ mol L⁻¹ s⁻¹. at what rate is nitrogen consumed? think about the stoichiometry. be sure to include units in your answer.


N₂ is consumed at the rate of_____ L⁻¹ s⁻¹

Answer 1

In the Haber process for ammonia production, N₂ is consumed at half the rate of NH₃ production. Given the NH₃ production rate of 6.29 x 10⁻⁵ mol/L/s, nitrogen is consumed at a rate of 3.145 x 10⁻⁵ mol/L/s.

Step-by-step explanation:

The reaction for the Haber process, the industrial production of ammonia, is N₂(g) + 3H₂(g) → 2NH₃(g). When considering the stoichiometry of the reaction, we can see that 1 mole of nitrogen reacts to form 2 moles of ammonia. If ammonia is produced at the rate of 6.29 x 10⁻⁵ mol L⁻⁹ s⁻⁹, we can use the stoichiometry to find out how quickly nitrogen is being consumed. Since the ratio of N₂ to NH₃ is 1:2 in the balanced equation, we divide the rate of ammonia production by 2 to find the rate at which nitrogen is consumed. Therefore, nitrogen is consumed at the rate of 3.145 x 10⁻⁵ mol L⁻⁹ s⁻⁹.

The reaction for the Haber process, which is the industrial production of ammonia, is represented by the equation: N₂(g) + 3H₂(g) → 2NH₃(g). The stoichiometry of the reaction tells us that for every 1 mole of nitrogen consumed, 2 moles of ammonia are produced. Therefore, the rate of nitrogen consumption is equal to half the rate of ammonia production. In this case, ammonia is produced at a rate of 6.29 x 10⁻⁵ mol L⁻¹ s⁻¹, so nitrogen is consumed at a rate of 3.15 x 10⁻⁵ mol L⁻¹ s⁻¹.