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

The stoichiometry of the reaction shows that 3 moles of H₂ are produced for every 2 moles of NH₃ consumed. Therefore, the rate of consumption of NH₃ is (2/3) times the rate of production of H₂, which is (2/3) * 0.030 mol L⁻¹s⁻¹ = 0.020 mol L⁻¹s⁻¹. Since NH₃ is being consumed, the rate is negative: -0.020 mol L⁻¹s⁻¹.

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

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