Just answers is necessary. Consider the reaction 2NO2O(g) rightarrow 2N2(g) + O2

Question

Just answers is necessary.

Consider the reaction 2NO2O(g) rightarrow 2N2(g) + O2(g) rate=k[N2O]. Calculate the time in seconds required for the concentration of N2O(g) to decrease from 0.75 M to 0.33 M. The rate constant for this reaction is k=6.8*10 -3 s-1 Based on the plot below what is the rate constant, k, for the dimerization of butadiene? The following reaction A + B rightarrow C is found to follow the rate law rate=k[A][B] when will a plot of ln[A] vs time yield a straight line? When the [B][A] when [B]=[A] never

Explanation / Answer

1) The given rxn is the first order rxn, hence

ln[Ao/At] = k*t

ln[0.75/0.33] = 6.8*10^(-3)*t

hence t = 120.55 seconds

3) For the graph problem,

the rate of rxn will be second order since 1/conc is givnig a straight plot

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