Question

The decomposition of Na2O5 to N2O5 to NO2 and O2 is first order, with a rate constant of 4.80x10^-4 at 45 degrees Celsius. a. If the initial concentration is 1.65x10^-2 mol/L, what is the concentration after 825 s? b. How long would it take for the concentration of N2O5 to decrease to 1.00x10^-2 from its initial value in a?

Name: the decomposition of na2o5 to n2o5 to no2 and o2 is first order with rate constant of 480x10 4 at 45 degrees celcius aif the initial concentration is 165x10 2 moll what is concentration afte 71542
Uploaded: 2022-06-02T14:42:24-08:00
Duration: 4 min 37 s
Channel: Shaiju T
Description: the decomposition of na2o5 to n2o5 to no2 and o2 is first order with rate constant of 480x10 4 at 45 degrees celcius aif the initial concentration is 165x10 2 moll what is concentration afte 71542

          The decomposition of Na2O5 to N2O5 to NO2 and O2 is first order, with a rate constant of 4.80x10^-4 at 45 degrees Celsius. 
a. If the initial concentration is 1.65x10^-2 mol/L, what is the concentration after 825 s?
b. How long would it take for the concentration of N2O5 to decrease to 1.00x10^-2 from its initial value in a?

Added by Julia A.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Shaiju T

06/02/2022

Step 1

We are dealing with a first-order reaction where the rate constant \(k = 4.80 \times 10^{-4} \, \text{s}^{-1}\) at \(45^\circ \text{C}\). The initial concentration of \(N_2O_5\) is \(1.65 \times 10^{-2} \, \text{mol/L}\). We need to find the concentration after Show more…

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The decomposition of Na2O5 to N2O5 to NO2 and O2 is first order, with a rate constant of 4.80x10^-4 at 45 degrees Celsius. a. If the initial concentration is 1.65x10^-2 mol/L, what is the concentration after 825 s? b. How long would it take for the concentration of N2O5 to decrease to 1.00x10^-2 from its initial value in a?