Half-Life of a Reaction. Consider the following reaction at 300 C: NO2(g) = NO(g) + 1/2 O2(g).
a. Describe what kinds of plots you would have to construct to determine if the reaction is first-order or second-order.
b. What would these plots look like and how would they allow you to determine the order of the reaction?
c. If the rate constant for the reaction at 300 C is found to be 0.543 M -1s-1, what is the half-life for the decomposition of NO2 if [NO2]o = 0.0100 M?
a,b) The type of plots are going to depend on the rate equations. The rate equations are:
1st order --> ln[R]t = ln[R]o - kt
2nd order --> 1/[R]t = 1/[R]o +kt
Notice these are of the form: y = ax +b
So, if you ...
This solution is provided in 215 words. It uses rate equations to determine the plots and order of reactions.