Question

N?O? decomposes to form NO? and O? with first-order kinetics and the rate constant, k, equals 5.89 x 10?³? How long does it take for the N?O? concentration to decrease from its initial value of 2.75 M to its final value of 1.85 M? 30.0 minutes 153 minutes 67.3 minutes

          N?O? decomposes to form NO? and O? with first-order kinetics and the rate constant, k, equals 5.89 x 10?³?
How long does it take for the N?O? concentration to decrease from its initial value of 2.75 M to its final value of 1.85 M?
30.0 minutes
153 minutes
67.3 minutes

N?O? decomposes to form NO? and O? with first-order kinetics and the rate constant, k, equals 5.89 x 10?³?
How long does it take for the N?O? concentration to decrease from its initial value of 2.75 M to its final value of 1.85 M?
30.0 minutes
153 minutes
67.3 minutes

Added by Jordi R.

Calculus: Early Transcendentals

James Stewart 8th Edition

Instant Answer

Solved by Expert Dj Tan

08/02/2022

Step 1

Given that the rate constant, k, is 5.89 x 10^(-3), the rate law for the decomposition of N2O5 can be written as: Rate = k[N2O5] where [N2O5] is the concentration of N2O5 at any given time. Since the reaction is first-order, the rate law simplifies to: Rate = Show more…

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N2O5 decomposes to form NO2 and O2 with first-order kinetics and the rate constant, k, equals 5.89 x 10^(-3). How long does it take for the N2O5 concentration to decrease from its initial value of 275M to its final value of 1.85M? 30.0 minutes 153 minutes 67.3 minutes Next NOs decomposes to form NO and O with first-order kinetics and the rate constant, k, equals 5.89 x 10^(-3). How long does it take for the NOs concentration to decrease from its initial value of 2.75M to its final value of 1.85M? 30.0 minutes 153 minutes 67.3 minutes Next