**Transcription for Educational Website:**### Reaction Table Analysis#### Reaction: \[ A + B \rightarrow AB \]This table presents the experimental data for the reaction between substances A and B to form AB. The concentrations of A and B, along with the reaction rate, are recorded for different trials.| Trial | [A] (M) | [B] (M) | Rate (M/s) ||-------|---------|---------|-------------|| 1 | 0.200 | 0.200 | 2.00 x 10⁻² || 2 | 0.400 | 0.200 | 8.00 x 10⁻² || 3 | 0.200 | 0.400 | 4.00 x 10⁻² |#### Key Observations:- **Trial 1**: Initial concentrations of A and B are both 0.200 M, resulting in a reaction rate of 2.00 x 10⁻² M/s.- **Trial 2**: The concentration of A is doubled to 0.400 M while keeping B constant at 0.200 M, leading to an increase in the reaction rate to 8.00 x 10⁻² M/s.- **Trial 3**: The concentration of B is doubled to 0.400 M, while A remains at 0.200 M, resulting in the rate increasing to 4.00 x 10⁻² M/s.#### Question:What is the overall order for the reaction above?Understanding how the concentration changes affect the rate will help determine the reaction order with respect to each reactant and the overall reaction order.

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Answered: A+B AB Trial [A] (M) (B) (M) Rate (M/…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Step 1) X(g) + Y(g) A(g) fast, reaches equilibrium (For Step 1, k1 = forward rate constant & k-1 = reverse rate constant.)Step 2) A(g) + Z(g) B(g) slow (k2 = rate constant) Step 3) B(g) P(g) fast (k3 = rate constant) a) What is the overall reaction? b) What is the rate law supported by this mechanism? Explain your answer. c) The following is experimental data found for this reaction: Initial [X] (M) Initial [Y] (M) Initial [Z] (M) Initial Rate (M/day) Exp 1 0.150 0.150 0.150 0.569 Exp 2 0.250 0.150 0.150 0.948 Exp 3 0.250 0.300 0.150 3.793 Exp 4 0.300 0.350 0.200 6.196 i) What is the experimentally determined rate law? ii) Determine the rate constant and include units. d) Does your experimentally determined rate law support the proposed mechanism? Explain your answer. e) ΔΔHo = -347 kJ/mol for the overall reaction. Draw a reasonable reaction profile for the proposed mechanism. Label your profile with the proper reactants,…
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Consider the following complex reaction: A + 2B → C whose initial rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: Trial [A](M) [B](M) Rate(M/s) 1 0.400 0.050 9.60 × 10−3 2 0.400 0.100 1.92 × 10−2 3 0.800 0.050 3.84 × 10−2 A) Write the rate law for this reaction. Use k to represent the rate constant. B) Solve for k in the above rate law. Express your answer to three significant figures. Include units for k.
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A+B AB Trial [A] (M) (B) (M) Rate (M/ 0.200 0.200 2.00x 10 2 0.400 0.200 8.00x10 0.400 4.00x10 3 0.200 What is the overall order for the reaction above? 1.