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For the reaction 2A + B → C, the values of initial rate at different reactant concentrations are given in the table below. The rate law for the reaction is: [A] (mol L^-1) | [B] (mol L^-1) | Initial Rate (mol L^-1 s^-1) 0.05 | 0.05 | 0.045 0.10 | 0.05 | 0.090 0.20 | 0.10 | 0.72
- Rate = k [A][B]
- Rate = k [A][B]^2
- Rate = k [A]^2 [B]^2
- Rate = k [A]^2 [B]
Correct answer: Rate = k [A][B]
Solution
The correct rate law is Rate = k [A][B] because the initial rate data shows that doubling the concentration of A while keeping B constant results in a proportional doubling of the rate, and similarly for B, indicating that both reactants are first order in the rate law.
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