The rate constant for this second-order reaction is 0.890 M–1·s–1 at 300 °C. A---> Products

Question

The rate constant for this second-order reaction is 0.890 M–1·s–1 at 300 °C.

A---> Products

How long (in seconds) would it take for the concentration of A to decrease from 0.800 M to 0.360 M?

Answer 1

Hi Jorstice,

 

Looking at this problem you are given one big clue: "This is a second order reaction."

 

From here, make a list of the bits of information that you have:

rate constant, k= 0.890 (1/M*s)

[A]₀= 0.800 M

[A]_t= 0.360 M

Temperature, T is 300 °C

time, t= ? seconds

 

Does the information above give you all variables you need to using the second order integrated rate law? Is the temperature important when using this rate law?

 

The second rate law is (1/[A]_t= kt + (1/[A]₀) for your convenience.