Consider the data presented from the following reaction: A(g) —> B(g)

Question

Consider the data presented from the following reaction: A(g) —> B(g):

time(sec): 0, 40, 80, 120, 160

[A](moles/liter): .100, .067, .045, .030, .020

a) determine if the reaction is of the 1st order or 2nd order using the appropriate data and graphs.

b) what is the value of the rate constant.

c) what is half-life of the reaction.

Answer 1

I can't plot data on this platform, but here is how you go about answering this question.

a) Make 2 plots of the data.

(1). plot ln[A] vs. time

(2). plot 1/[A] vs. time

If plot (1) is linear, it is FIRST order

If plot (2) is linear, it is SECOND order

b) if first order, rate constant k = -slope of the line

if second order, rate constant k = slope of the line

c) if first order, half life = 0.692/k

if second order, half life = 1/k[A]₀ = 1/0.1k