Consider the hypothetical reaction: A + B +2C -------> 2D + 3E, where the rate law...
Consider the hypothetical reaction:
A + B +2C -------> 2D + 3E, where the rate law is:
Rate = -delta[A] / delta t = k[A][B]^2.
An experiment is carried out where [A]0 = 1.0*10^-2M, [B]0 = 3.0M, [C]0 = 2.0M. The reaction is started, and after 8.0 seconds, the concentration of A is 3.8*10^-3M.
a) Calculate the value of k for the reaction.
b) Calculate the half-life for this experiment.
c) Calculate the concentration of A after 13.0 seconds
d) Calculate the concentration of C after 13.0 seconds
I know that this is a pseudo-first-order reaction, but I don't know how to calculate the half-life and concentrations after the k is determined.
Thank you.
Homework Answers
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