The decomposition of nitrogen dioxide to nitrogen and oxygen is second-order wit

Question

The decomposition of nitrogen dioxide to nitrogen and oxygen is second-order with a rate constant k= 12.5 M-1 s-1. What is the half-life for the reaction if [NO2]0 = 0.00260 M? determine the order of the graph. If the mechanism for the reaction 2 NO + O2 rightarrow 2 NO2 is NO + NO rightarrow N202(fast equilibrium) N202 + O2 rightarrow 2 NO2 (slow) what is the rate law for each elementary process? What is the rate law of this reaction? At equilibrium all chemical processes have ceased the rate of the forward reaction equals that of the reverse the rate constant for the forward reaction equals that of the reverse, and the rate constant for forward reaction equals that of the reverse none of these

Explanation / Answer

14)for a second order reaction,

1/[A] - 1/[Ao] = kt

or 2/0.0026 - 1/0.0026 = 12.5*t

or t=30.77 s

17) the correct option is B (since the rate of the forwards reaction is equal to that of the backward reaction)

18) since the coefficients of the reactants, are thrice of that of the first reaction and the second reaction is inverse of the first reaction,

the value oft he equilibrium constant is K= (4.22*10^-3)^-3

=1.33*10^7

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