Consider the reaction: A + B −> C
If it is 2nd order in A and 0 order in B, a plot of [B]−1 vs time will be...
a. linear and negative
b. exponential and negative
c. linear and positive
d. equal to zero
e. exponential and positive
Here is your answer.
http://www.chm.davidson.edu/vce/kinetics/integratedratelaws.html
To determine the plot of [B]^-1 vs time for a reaction that is 2nd order in A and 0 order in B, we need to understand the rate equation of the reaction.
The rate equation for a reaction is given by:
Rate = k[A]^m[B]^n
Where k is the rate constant, [A] and [B] are the concentrations of reactants A and B, and m and n are the orders of the reaction with respect to A and B, respectively.
In this case, it is given that the reaction is 2nd order in A and 0 order in B. So the rate equation becomes:
Rate = k[A]^2[B]^0
Simplifying this, we get:
Rate = k[A]^2
Since the concentration of B does not affect the rate of the reaction, plotting [B]^-1 vs time would yield a constant value because [B] does not change over time.
Therefore, the correct answer is:
d. equal to zero