Answer:
b
Explanation:
because it is products /reactants :)
Answer:
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:
<em>3NO(g) → N₂O(g) + NO₂(g).</em>
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.
<em>1) The rate of the overall reaction is?</em>
The rate of the overall reaction = Δ[N₂O]/Δt = 0.015 mol/L.s.
<em>2) The rate of change for NO is?</em>
The rate of change for NO = - Δ[NO]/Δt.
∵ -1/3 Δ[NO]/Δt = Δ[N₂O]/Δt.
<em>∴ The rate of change for NO = - Δ[NO]/Δt = 3 Δ[N₂O]/Δt </em>= 3(0.015 mol/L.s) = <em>0.045 mol/L.s.</em>
The phosphorous cycle does not include an atmospheric component because phosphorous does not cycle through the atmosphere. In comparison, important processes of the carbon and nitrogen cycle occur in the atmosphere
I believe it should be A. Increased reaction rate due to the increased number of collisions between particles.
