Hey there! I have these two questions for my chemistry class, and I am a little confused on how I should go about solving them. If someone could give me the steps necessary to solve these problems I would be most appreciative.
1.) p-Toluenesulfinic acid undergoes a second-order redox action at room temperature.
a.) The value of the rate constant k for the reaction is 0.141 L mol^-1 min^-1. What is the half-life of p-Toluenesulfinic acid?
b.) If the initial concentration of p-Toluenesulfinic acid is 0.355 M, at what time will its concentration be 0.0355 M?
Sure! I can help you with these chemistry questions.
Let's start with the first question:
a.) To find the half-life of p-Toluenesulfinic acid, we can use the second-order rate equation:
1/t = k[A]
Where t is the half-life, k is the rate constant, and [A] is the initial concentration of the reactant (p-Toluenesulfinic acid in this case).
We can rearrange the equation to solve for t:
t = 1 / (k[A])
Given that k = 0.141 L mol^-1 min^-1, we need the value of [A]. Unfortunately, the question didn't provide it directly, so we need more information to proceed.
b.) To determine the time at which the concentration of p-Toluenesulfinic acid will be 0.0355 M, we can use the integrated rate law for a second-order reaction:
1/[A] = kt + 1/[A]0
Where [A] is the final concentration, [A]0 is the initial concentration, k is the rate constant, and t is the time.
We can rearrange the equation to solve for t:
t = (1/[A] - 1/[A]0) / k
Given that [A]0 = 0.355 M, [A] = 0.0355 M, and k = 0.141 L mol^-1 min^-1, we can substitute these values into the equation to find the time.
Please note that to completely answer these questions, we need to know the initial concentration of p-Toluenesulfinic acid for part a. If you have that information, please provide it, and we can proceed with the calculation.