When the reaction 3 no(g) → n2o(g) + no2(g) is proceeding under conditions such that 0.015 mol/l of n2o is being formed each second, the rate of the overall reaction is ? and the rate of change for no is ?

1) The rate of the overall reaction = Δ[N₂O]/Δt = 0.015 mol/L.s.

2) The rate of change for NO = - Δ[NO]/Δt = 3 Δ[N₂O]/Δt  = 0.045 mol/L.s.

Explanation:

3NO(g) → N₂O(g) + NO₂(g).

The rate of the reaction = -1/3 Δ[NO]/Δt = Δ[N₂O]/Δt = Δ[NO₂]/Δt.

Given that: Δ[N₂O]/Δt = 0.015 mol/L.s.

1) The rate of the overall reaction is?

The rate of the overall reaction = Δ[N₂O]/Δt = 0.015 mol/L.s.

2) The rate of change for NO is?

The rate of change for NO = - Δ[NO]/Δt.

∵ -1/3 Δ[NO]/Δt = Δ[N₂O]/Δt.

∴ The rate of change for NO = - Δ[NO]/Δt = 3 Δ[N₂O]/Δt = 3(0.015 mol/L.s) = 0.045 mol/L.s.

thats how its supposed to be

it would be a gas formation