The reaction 2 NO2 2 NO + O2 has the rate constant k = 0.63 M–1s- 1. (a) Based on the units for k, is the reaction first or second order in NO2? (b) If the initial concentration of NO2 is 0.100 M, how would you determine how long it would take for the concentration to decrease to 0.025 M?

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ultramarinehornet528Lv1

26 Apr 2020

The reaction 2 NO₂ 2 NO + O₂ has the rate constant k = 0.63 M^–¹s^{- 1}. (a) Based on the units for k, is the reaction first or second order in NO₂? (b) If the initial concentration of NO₂ is 0.100 M, how would you determine how long it would take for the concentration to decrease to 0.025 M?

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20 May 2020

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The gas-phase decomposition of NO₂, 2 NO₂(g) 2 NO(g) + O₂(g), is studied at 383 °C, giving the following data:

(a) Is the reaction first order or second order with respect to the concentration of NO₂? (b) What is the rate constant? (c) Predict the reaction rates at the beginning of the reaction for initial concentrations of 0.200 M, 0.100 M, and 0.050 M NO₂.

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1. The decomposition of NO2 to yield NO and O2 is second order in NO2. If k has a value of 755 M-1 sec-1 at 603 K and 4020 M-1 sec-1 at 652 K, calculate the activation energy and the frequency factor.

2. In the above example, if you start with a 1.0 M concentration of NO2 at 603K, how long will it take until only one fourth of the NO2 remains? need answer to part 2

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