1
Question
Given the following information, determine which elementary reaction has the highest frequency (occurrence) with the lowest success of molecular collisions.
Rate law k(s−1) 1 rate=k[A]1[B]3[C]0 3.16×10−4 2 rate=k[A]0[B]2[C]1 6.42×10−5 3 rate=k[A]1[B]1[C]1 1.26×10−3 4 rate=k[A]1[B]2[C]1
7.95×10−4
Given the following information, determine which elementary reaction has the highest frequency (occurrence) with the lowest success of molecular collisions.
| Rate law | k(s−1) | |
| 1 | rate=k[A]1[B]3[C]0 | 3.16×10−4 |
| 2 | rate=k[A]0[B]2[C]1 | 6.42×10−5 |
| 3 | rate=k[A]1[B]1[C]1 | 1.26×10−3 |
| 4 | rate=k[A]1[B]2[C]1 | 7.95×10−4 |
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Solution
The correct option is D Reaction 1.
Arrhenius Equation,
k=Ae−EaRT
From the equation, it can be seen that higher the activation energy lower is the rate constant.
For highest activation energy there is the highest frequency of occurrence at lowest success of molecular collisions..
Hence, the correct option is A
Arrhenius Equation,
k=Ae−EaRT
From the equation, it can be seen that higher the activation energy lower is the rate constant.
For highest activation energy there is the highest frequency of occurrence at lowest success of molecular collisions..
For highest activation energy there is the highest frequency of occurrence at lowest success of molecular collisions..
Hence, the correct option is A
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