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4. Consider the first-order decomposition reaction of N₂O5 as shown below: N₂O5 2NO2+ - 0₂ 2 At 45°C, the reaction began with an initial N₂O5 concentration of 1.00 mol L-1. After 3 h, the N2O5 concentration decreased to 1.21 x 10-3 mol L-1. Calculate: (a) the half-life of N₂O5 at 45 °C (in min). (b) the time required for N₂O5 concentration to change from 0.250 mol L-1 to 0.010 mol L-¹.

4. Consider the first-order decomposition reaction of N₂O5 as shown below: N₂O5 2NO2+ - 0₂ 2 At 45°C, the reaction began with an initial N₂O5 concentration of 1.00 mol L-1. After 3 h, the N2O5 concentration decreased to 1.21 x 10-3 mol L-1. Calculate: (a) the half-life of N₂O5 at 45 °C (in min). (b) the time required for N₂O5 concentration to change from 0.250 mol L-1 to 0.010 mol L-¹.

Chemistry
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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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4. Consider the first-order decomposition reaction of N₂O5 as shown below: N2O5 → 2NO2 + O2 At 45°C, the reaction began with an initial N₂O5 concentration of 1.00 mol L-1. After 3 h, the N2O5 concentration decreased to 1.21 x 10-3 mol L-1. Calculate: (a) the half-life of N₂O5 at 45 °C (in min). (b) the time required for N₂O5 concentration to change from 0.250 mol L-¹ to 0.010 mol L-¹1¹.
Transcribed Image Text:4. Consider the first-order decomposition reaction of N₂O5 as shown below: N2O5 → 2NO2 + O2 At 45°C, the reaction began with an initial N₂O5 concentration of 1.00 mol L-1. After 3 h, the N2O5 concentration decreased to 1.21 x 10-3 mol L-1. Calculate: (a) the half-life of N₂O5 at 45 °C (in min). (b) the time required for N₂O5 concentration to change from 0.250 mol L-¹ to 0.010 mol L-¹1¹.
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