using the following mechanism, determine the rate law.
2A <-- --> B+C
B+D --> E
2A + D --> C + E
k=?
please indicate which k you are using for which equation
To determine the rate law for each reaction and the associated rate constant (k), let's break down the given mechanism and examine each step individually.
Step 1: 2A ⇌ B + C (Reaction 1)
The rate law for the forward reaction would be written as: rate = k1[A]², where k1 is the rate constant associated with this step and [A] represents the concentration of A.
The rate law for the reverse reaction (B + C → 2A) would be: rate = k-1[B][C], where k-1 is the rate constant for the reverse reaction.
Step 2: B + D → E (Reaction 2)
The rate law for this reaction can be expressed as: rate = k2[B][D], where k2 is the rate constant associated with this reaction, [B] represents the concentration of B, and [D] represents the concentration of D.
Step 3: 2A + D → C + E (Reaction 3)
The rate law for this reaction would be: rate = k3[A]²[D], where k3 is the rate constant associated with this step, [A] represents the concentration of A, and [D] represents the concentration of D.
Now that we have identified the rate laws for each reaction, we can determine the values of the rate constants (k) specific to each equation.
To find the values of k1, k-1, k2, and k3, experimental data is required. The rate laws can be compared with the experimental rate data to determine the specific values of the rate constants for each reaction.