Consider the following mechanism.
Step1: 2A--->B (SLOW)
Step2: B+C--->D (fast)
Overaall: 2A+C--> D
Determine the rate law for the overall reaction (where the overall rate constant is represented as k).
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To determine the rate law for the overall reaction, we need to consider the rate-determining step, which is the slowest step in the mechanism. In this case, Step 1 (2A → B) is the slow step.
The rate law for the slow step can be determined by looking at the reactants involved in that step. In Step 1, there are two A molecules reacting to form B. Therefore, the rate law for Step 1 is rate = k[ A ]^2, where k is the rate constant for the slow step.
Since the overall reaction involves the consumption of 2 A molecules and 1 C molecule to form D, the rate law for the overall reaction can be expressed as:
rate = k[ A ]^2 [ C ]
So, the rate law for the overall reaction is rate = k[ A ]^2 [ C ].