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 0.150 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><sup> </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 0.150 M. A) 3.34 B) 0.0880 C) 1.01 D) 0.299 E) 5.19

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 0.150 M.

Quizplus · Accepted Answer

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 0.150 M.

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