e rate law for the reaction described in equation 4 is second order in [N2O]. The reaction was carried out at 900 K with an initial concentration of N2O (g) of 2.0 x 10-2 M. It took 4500 seconds for [N2O] to fall to half its initial value. Determine the value of the rate constant for this reaction. 2 N2O (g) → 2 N2 (g) + O2 (g) step by step please

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