For a reaction, 2A + B -->C , the rate law is, rate = k × [A]^2 × [B]. If the rate constant of the reaction is 3.74 × 10^(-2) M^(-1) s^(-1). Calculate the rate of the reaction when the concentrations of A, B, and C are 0.108 M, 0.132 M, and 0.124 M, respectively.
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Explanation:
The rate law for the given reaction is \( \text{rate} = k \times [A]^2 \times [B] \), where \( k = 3.74 \times 10^{-2} \, \text{M}^{-1} \, \text{s}^{-1} \).
Substitute the given concentrations into the rate law:
\[ \text{rate} = (3.74 \times 10^{-2} \, \text{M}^{-1} \, \text{s}^{-1}) \times (0.108 \, \text{M})^2 \times (0.132 \, \text{M}) \]
Calculate the result to find the rate of the reaction.