The decomposition of N2O5 to NO2 and O2 is first order, with a rate constant of 4.80 × 10-4/s at 45°C. If the initial concentration of N2O5 is 7.98×10-2 mol/L, what is the concentration of N2O5 after 503 s?How long would it take for the concentration of N2O5 to decrease to 1.00 × 10-2 mol/L from an initial concentration of 7.98×10-2 mol/L?

Given reaction The decomposition of N2O5 N2O5 ----> NO2 + O2 Rate Constant = k = 4.80 * 10-4 s-1…

Answered: he decomposition of N2O5 to NO2 and O2…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The decomposition of N₂O₅ to NO₂ and O₂ is first order, with a rate constant of 4.80 × 10^-4/s at 45°C. If the initial concentration of N₂O₅ is 7.98×10^-2 mol/L, what is the concentration of N₂O₅ after 503 s?

How long would it take for the concentration of N₂O₅ to decrease to 1.00 × 10^-2 mol/L from an initial concentration of 7.98×10^-2 mol/L?

Expert Solution

Step 1

Given reaction

The decomposition of N₂O₅

N₂O₅ ----> NO₂ + O₂

Rate Constant = k = 4.80 * 10^-4 s^-1

Initial concentration [N₂O₅]₀ = 7.98×10^-2 mol/L

Concentration at t =503 s = [N₂O₅]_t = To be determined

Initial concentration [N₂O₅]₀ = 7.98×10^-2 mol/L

Concentration at time t = [N₂O₅]_t = 1.00 × 10^-2 mol/L

Time =t = To be determined

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