Consider the following first order reaction for the decomposition of dinitrogen pentoxide:
N₂O₅(g) 2 NO₂ (g) + O₂(g) At 70 C, the rate constant, k , for this reaction equals 6.82 * 10^-3 s^-1 . If the initial concentration of N₂O₅ equals 0.0125 M, how long would it take for the concentration of N₂O₅ to reduce to 0.00500 M?

Question

Consider the following first order reaction for the decomposition of dinitrogen pentoxide:
N₂O₅(g)

Consider the following first order reaction for the decomposition of dinitrogen pentoxide: N₂O<sub>5</sub>(g) 2 NO₂ (g) + O₂(g) At 70 C, the rate constant, k , for this reaction equals 6.82 * 10<sup>-3</sup> s<sup>-1</sup> . If the initial concentration of N₂O<sub>5</sub> equals 0.0125 M, how long would it take for the concentration of N₂O<sub>5</sub> to reduce to 0.00500 M? A) 6.25×10<sup> - 3</sup> sec B) 58.3 sec C) 102 sec D) 134 sec E) 177 sec

2 NO₂ (g) + O₂(g) At 70 C, the rate constant, k , for this reaction equals 6.82 * 10^-3 s^-1 . If the initial concentration of N₂O₅ equals 0.0125 M, how long would it take for the concentration of N₂O₅ to reduce to 0.00500 M?

Quizplus · Accepted Answer

The Answer of Consider the following first order reaction for the decomposition of dinitrogen pentoxide: N₂O₅(g) 2 NO₂ (g) + O₂(g) At 70 C, the rate constant, k , for this reaction equals 6.82 * 10^-3 s^-1 . If the initial concentration of N₂O₅ equals 0.0125 M, how long would it take for the concentration of N₂O₅ to reduce to 0.00500 M?

Consider the Following First Order Reaction for the Decomposition of Dinitrogen