Consider the reaction 2NH₃(g) → N₂(g) + 3H₂(g)
If the rate Δ[H₂]/Δt is 0.030 mol L⁻¹s⁻¹, then Δ[NH₃ ]/Δt is

Question

Consider the reaction 2NH₃(g) → N₂(g) + 3H₂(g) If the rate Δ[H₂]/Δt is 0.030 mol L⁻¹s⁻¹, then Δ[NH₃ ]/Δt is

Quizplus · Accepted Answer

Given the reaction 2NH₃(g) → N₂(g) + 3H₂(g), the rate of disappearance of NH₃ is linked to the rate of appearance of H₂ by a factor of 3 (since 3 moles of H₂ are produced for every 1 mole of NH₃ that reacts). Therefore, if Δ[H₂]/Δt = 0.030 mol/L/s, then Δ[NH₃]/Δt = -0.030 mol/L/s / 3 = -0.010 mol/L/s, which corresponds to choice D, not C as initially indicated. My correction is based on the stoichiometry of the reaction, indicating an error in my initial response. The correct answer should be D, reflecting the stoichiometric relationship between the reactants and products.

Consider the Reaction 2NH3(g) → N2(g) + 3H2(g)

Consider the Reaction 2NH₃(g) → N₂(g) + 3H₂(g)