| \[2A+B\to D+E\] |
| \[A+B\to C+D\left( slow \right)\] |
| \[A+C\to E\left( fast \right)\] |
| The rate law expression for the reaction is: |
A) \[r=k{{\left[ A \right]}^{2}}\left[ B \right]\]
B) \[r=k\left[ A \right]\left[ B \right]\]
C) \[r=k{{\left[ A \right]}^{2}}\]
D) \[r=k\left[ A \right]\left[ C \right]\]
Correct Answer: B
Solution :
[b] From slow reaction Rate =k[A][B]
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