The gas phase decomposition of NO₂(g)2NO₂(g) → 2NO(g) + O₂(g)obeys the second order rate law, Rate = K[NO]², with a rate constant k= 0.543 M¹s¹ at 300 °C. Starting with [NO₂] = 0.250 M, how long will ittake for the [NO₂] to decrease to 5.00% of its starting value?

we have to determine the time taken for concentration of NO2 to decreases to 5.00% of the initial…

The gas phase decomposition of NO₂(g) 2NO₂(g) → 2NO(g) + O₂(g) obeys the second order rate law, Rate = K[NO₂1², with a rate constant k = 0.543 M¹¹s¹ at 300 °C. Starting with [NO₂] = 0.250 M, how long will it take for the [NO₂] to decrease to 5.00% of its starting value?

The gas phase decomposition of NO₂(g) 2NO₂(g) → 2NO(g) + O₂(g) obeys the second order rate law, Rate = K[NO₂1², with a rate constant k = 0.543 M¹¹s¹ at 300 °C. Starting with [NO₂] = 0.250 M, how long will it take for the [NO₂] to decrease to 5.00% of its starting value?

Chemistry

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ISBN:9781305957404

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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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Question

The gas phase decomposition of NO₂(g)
2NO₂(g) → 2NO(g) + O₂(g)
obeys the second order rate law, Rate = K[NO]², with a rate constant k
= 0.543 M¹s¹ at 300 °C. Starting with [NO₂] = 0.250 M, how long will it
take for the [NO₂] to decrease to 5.00% of its starting value?

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