Solution: What is the rate law for the following mechanism in terms of the overall rate constant k? Step 1: A + B ↔ C (fast) Step 2: B + C → D (slow)

Problem

What is the rate law for the following mechanism in terms of the overall rate constant k? 

Step 1: A + B ↔ C (fast) 

Step 2: B + C → D (slow)

Solution

We’re asked to determine the overall rate constant K for the given two steps mechanism.

When a reaction mechanism is given, the rate law will depend on reactants and products in the slow step.

Rate law only involves the reactants
 The coefficients of the reactants in the slow step are the order of the reaction with respect to that reactant
 Rate Law has a general form of:

Rate Law=kXaYb

Where

k = rate constant

X & Y = reactants

a & b = reactant orders


 The equilibrium constant has a general form of:

 Kr=productsreactants


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