First order reactions are important in chemical reactions as well as in pharmaco

Question

First order reactions are important in chemical reactions as well as in pharmacology. First order refers to the rate of a reaction. If the reaction is AB, then stating that it is first order implies that rate=k*[A], where k is some constant and [A] is the concentration of A. Which of the following does not hold true for such an order reaction?

A) The slope of log[A] over time is linear

B) Half-life depends on the concentration of A

C) If [A] doubles, so will the rate of the reaction

D) Changing [B] will have no impact on the rate

Explanation / Answer

integrated rate law for 1st order reaction

log[A] = log[A]o - k*t

So, log[A] vs t is linear

half life of 1st order reaction = 0.693/K

So, half life does not depend on concentration of A

rate = k [A]

so, when [A] doubles, rate will double

[B] is product, changing it will not have any impact on rate

Answer: B

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