Nitrosyl bromide decomposes by the reaction 2 NOBr( g ) 2 NO( g ) + Br 2 ( g ).

ID: 974783 • Letter: N

Question

Nitrosyl bromide decomposes by the reaction 2 NOBr(g) 2 NO(g) + Br2(g). Show that the following data are consistent with a second-order reaction and determine the second-order rate constant for the reaction.

the rate law is: rate = k . [NOBr]^{2}

Students may do this by plotting the data three different ways.
For each plot, time goes on the x-axis.
A zero-order reaction is linear when [NOBr] on the y-axis.
A first-order reaction is linear when ln[NOBr] is on the y-axis.
A second-order reaction is linear when 1/[NOBr] is on the y-axis.

What is the value of the rate constant at the temperature of the experiment?

t 0 5 10 15 40 65 s [NOBr] 0.0653 0.0514 0.0424 0.0361 0.0207 0.0145 M

Explanation / Answer

For a second order reaction

-dCA/dt= KCA2

when integrated at t=0 CA=CAO and t= t, CA=CA

1/CA= 1/CAO+ Kt

where CA= concentration of NOBr any time, K is rate constant

so a plot of 1/CA vs t gives slope of K ,the rate constant and the intercept the initial concentration

The plot of 1/CA and t is shown below

The equation of best fit as shown is 1/CA= 0.825t+15.32

the slope is K=0.825/M.sec and intercept = 1/CAO= 15.32 and CAO= 0.0653

Navigate

Nitrosyl bromide decomposes according to the following equation: 2NOBr(g) -><- 2

Nitrosyl bromide, NOBr, is formed in the reaction of nitric oxide, NO, with brom

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.

Nitrosyl bromide decomposes by the reaction 2 NOBr( g ) 2 NO( g ) + Br 2 ( g ).

Question

Explanation / Answer

Related Questions

Navigate