Suppose that the reaction in Example 20-8 is first order with a rate constant of 0.12 min^-1. Starting with [A]₀ = 1.00 M, will the curve for [A] versus t for the first-order reaction cross the curve for the second-order reaction at some time after t = 0? Will the two curves cross if [A]₀ = 2.00 M? In each case, if the curves are found to cross, at what time will this happen?

Example 20-8

An alternative mechanism of the reaction 2 NO(g) + O₂(g) → 2 NO₂(g) follows. Show that this mechanism is consistent with the rate law, equation (20.24).

Eq. 20.24

Transcribed Image Text:

Fast: Slow: Overall: NO(g) + O₂(g) 0₂(g) NO3(g) + NO(g) 2 NO(g) + O₂(g) K-1 k₂ NO3(g) 2 NO₂(g) 2 NO2(g)