Question

Consider the following reaction: 2 N2O(g) → 2 N2(g)+O2(g)

Part A Express the rate of the reaction in terms of the change in concentration of each of the reactants and products. Express the rate of the reaction in terms of the change in concentration of each of the reactants and products.Rate=12Δ[N2O]Δt=−12Δ[N2]Δt=Δ[O2]ΔtRate=Δ[N2O]Δt=12Δ[N2]Δt=−12Δ[O2]ΔtRate=−Δ[N2O]Δt=−12Δ[N2]Δt=12Δ[O2]ΔtRate=−12Δ[N2O]Δt=12Δ[N2]Δt=Δ[O2]Δt Part B In the first 14.0  s of the reaction, 1.9×10−2  mol of O2 is produced in a reaction vessel with a volume of 0.460  L . What is the average rate of the reaction over this time interval? Express your answer using two significant figures. Part C Predict the rate of change in the concentration of N2O over this time interval. In other words, what is Δ[N2O]Δt? Express your answer using two significant figures.

Answer 1

Part(A)

(d) is correct option.

Part(b)

Rate of reaction = 0.019/0.46×14

Rate = 0.0030 M/s

Part(c)

∆[N2O]/∆t = 0.0060 M/s