Multiple Choice
For the zeroth-order reaction: A → products, what will happen to the rate of reaction if the concentration of A is doubled?
15. Chemical Kinetics
Intro to Chemical Kinetics
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Which of the following linear plots do you expect for a reaction A → products if the reaction follows first-order kinetics?
A
1/[A] vs. time
B
ln[A] vs. time
C
[A] vs. time
D
Rate vs. [A]
Verified step by step guidance1
Understand that first-order kinetics means the rate of reaction is directly proportional to the concentration of one reactant.
Recall the integrated rate law for a first-order reaction: \( \ln[A] = -kt + \ln[A]_0 \), where \( [A] \) is the concentration of reactant A at time t, \( k \) is the rate constant, and \( [A]_0 \) is the initial concentration.
Recognize that the integrated rate law equation \( \ln[A] = -kt + \ln[A]_0 \) is in the form of a straight line \( y = mx + c \), where \( y = \ln[A] \), \( m = -k \), \( x = t \), and \( c = \ln[A]_0 \).
Identify that plotting \( \ln[A] \) versus time \( t \) will yield a straight line with a slope of \(-k\) and a y-intercept of \( \ln[A]_0 \).
Conclude that for a first-order reaction, the correct linear plot is \( \ln[A] \) versus time, as it will produce a straight line, confirming the reaction order.
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