객관식
For the reaction x + 2 y → xy₂, if the reaction occurs in a single elementary step as proposed, what is the correct rate law?
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15. Chemical Kinetics
Rate Law
객관식
Using the information in the table below, what is the correct rate law for the reaction 2 A(g) + B(g) → C(g) + D(g)? | Experiment | [A] (M) | [B] (M) | Initial Rate (M/s) | |------------|--------|--------|--------------------| | 1 | 0.10 | 0.10 | 2.0 × 10^{-3} | | 2 | 0.20 | 0.10 | 4.0 × 10^{-3} | | 3 | 0.10 | 0.20 | 2.0 × 10^{-3} | Which of the following is the correct rate law?
A
rate = k[A]
B
rate = k[A][B]
C
rate = k[B]
D
rate = k[A]^2
검증된 단계별 안내1
Identify the general form of the rate law for the reaction: \(\text{rate} = k [A]^m [B]^n\), where \(m\) and \(n\) are the reaction orders with respect to A and B, respectively.
Compare experiments 1 and 2 to determine the order with respect to A: The concentration of A doubles from 0.10 M to 0.20 M while B remains constant at 0.10 M. Observe how the initial rate changes between these two experiments.
Use the rate ratio from experiments 1 and 2 to find the order \(m\) with respect to A by setting up the equation: \(\frac{\text{rate}_2}{\text{rate}_1} = \left(\frac{[A]_2}{[A]_1}\right)^m\). Solve for \(m\).
Compare experiments 1 and 3 to determine the order with respect to B: The concentration of B doubles from 0.10 M to 0.20 M while A remains constant at 0.10 M. Observe how the initial rate changes between these two experiments.
Use the rate ratio from experiments 1 and 3 to find the order \(n\) with respect to B by setting up the equation: \(\frac{\text{rate}_3}{\text{rate}_1} = \left(\frac{[B]_3}{[B]_1}\right)^n\). Solve for \(n\). Then, write the final rate law using the determined orders.
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