At elevated temperatures, nitrogen dioxide decomposes to nitrogen oxide and oxygen: NO₂(g) → NO (g) + O₂(g)
The reaction is second order in NO₂ with a rate constant of 0.543 M^-1s^-1at 300 °C. If the initial [NO₂] is 0.260 M, it will take ________ s for the concentration to drop to 0.075 M.

Question

At elevated temperatures, nitrogen dioxide decomposes to nitrogen oxide and oxygen: NO₂(g) → NO (g) +

At elevated temperatures, nitrogen dioxide decomposes to nitrogen oxide and oxygen: NO<sub>2 </sub>(g) → NO (g) + O<sub>2 </sub>(g) The reaction is second order in NO<sub>2</sub> with a rate constant of 0.543 M<sup>-1</sup>s<sup>-1</sup>at 300 °C. If the initial [NO<sub>2</sub>] is 0.260 M, it will take ________ s for the concentration to drop to 0.075 M. A) 3.34 B) 0.0880 C) 2.29 D) 0.299 E) 17.5

O₂(g)
The reaction is second order in NO₂ with a rate constant of 0.543 M^-1s^-1at 300 °C. If the initial [NO₂] is 0.260 M, it will take ________ s for the concentration to drop to 0.075 M.

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The Answer of At elevated temperatures, nitrogen dioxide decomposes to nitrogen oxide and oxygen: NO₂(g) → NO (g) + O₂(g) The reaction is second order in NO₂ with a rate constant of 0.543 M^-1s^-1at 300 °C. If the initial [NO₂] is 0.260 M, it will take ________ s for the concentration to drop to 0.075 M.

At Elevated Temperatures, Nitrogen Dioxide Decomposes to Nitrogen Oxide and Oxygen