Step-by-step explanation:
We are given the following reaction:
2 NO (g) + O₂ (g) ----> 2 NO₂ (g)
We know its rate law for this reaction.
rate = k [NO]² * [O₂]
We have to calculate the average value of the rate constant calculated from the three data sets.
We can replace the values in the rate expression for each trial and calculate for each of them the rate constant.
rate₁ = k₁ [NO]₁² * [O₂]₁
k₁ = rate₁/([NO]₁² * [O₂]₁)
k₁ = 1.41*10^(-2)/((0.0126)²*0.0125)
k₁ = 7.11 * 10^3
k₂ = rate₂/([NO]₂² * [O₂]₂)
k₂ = 1.13*10^(-1)/((0.0252)²*0.0250)
k₂ = 7.12 * 10^3
k₃ = rate₃/([NO]₃² * [O₂]₃)
k₃ = 5.64 * 10^(-2)/((0.0252)²*0.0125)
k₃ = 7.11 *10^3
Finally we have to average the three values that we obtained.
k = (k₁ + k₂ + k₃)/3
k = (7.11 * 10^3 + 7.12 * 10^3 + 7.11 * 10^3)/3
k = 7.11 * 10^3
Answer: k = 7.11 * 10^3 = 7110