The equation A + 2 B = C + D describes an elementary reaction, which takes place in a single step. Thus, the rate law must be
a. rate = k(A]2
b. rate = k(B]2
c. rate = k(A][B]
d. rate = k(A][B]2
e. none of the above represents the rate law for this elementary reaction.
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d. However, such three-body reactions are rare. They usually proceed in a number of steps that involve unstable intermediate species.
To determine the rate law for an elementary reaction, you need to look at the stoichiometric coefficients of the reactants in the balanced equation. In this case, the stoichiometric coefficients are 1 for A, 2 for B, 1 for C, and 1 for D.
The rate law would typically be in the form:
rate = k[A]^m[B]^n
where [A] and [B] represent the concentrations of A and B respectively, k is the rate constant, and m and n are the reaction orders with respect to A and B.
Looking at the given equation A + 2B = C + D, we can see that the rate is not directly proportional to the concentration of A, B, or both. Since the reaction is described in a single step, we can conclude that the answer is e. none of the above represents the rate law for this elementary reaction.
In summary, the rate law for this elementary reaction cannot be determined solely based on the given equation. More information is needed to determine the specific rate law.