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## Homework Statement

Consider the following reaction

NOBr (g) → NO (g) + ½ Br2 (g)

The table below gives the time-dependent concentration of NOBr. Using this data,

determine, if the reaction is first- or second-order, with respect to NOBr. Give the rate

equation and determine the rate constant. To do this you’ll need to generate two plots,

and be sure to explain your reasoning. Then determine the half-live and lifetime for

NOBr. Watch your units! (7 marks)

t/s [NOBr]/mol dm-3

0.0 0.0250

6.2 0.0191

10.8 0.0162

14.7 0.0144

20.0 0.0125

24.6 0.011

## Homework Equations

t

_{1/2}= ln2/k

_{r}

## The Attempt at a Solution

So I've been trying to work through this question for about an hour and a half and can't for the life of me figure out how to even start it off. I know I need to determine the order of the reaction first but can't even figure that out. If someone could give me two or three steps to get me going that would be great.

(I've made a graph of the time vs. concentration)