**Question 2 (15 points)**The initial rates listed in the following table were determined for the reaction:\[ 2 \text{NO} (g) + \text{Cl}_2 (g) \rightarrow 2 \text{NOCl} (g) \]| Trial | Initial [NO] (M) | Initial [Cl\(_2\)] (M) | Initial Rate of Consumption of Cl\(_2\) (M/s) ||-------|------------------|-----------------------|--------------------------------------------|| 1 | 0.13 | 0.20 | 1.0×10\(^\text{−2}\) || 2 | 0.26 | 0.20 | 4.0×10\(^\text{−2}\) || 3 | 0.13 | 0.10 | 5.0×10\(^\text{−3}\) |**Questions:**a. What is the rate law?b. What is the value of the rate constant, \( k \)?c. What is the initial rate when the initial concentrations of both reactants are 0.12 M?---### Explanation:#### Rate Law:The rate law for a chemical reaction is an equation that links the reaction's rate with the concentrations or pressures of the reactants and constant parameters (normally rate coefficients and partial reaction orders).For this reaction:\[ 2 \text{NO} (g) + \text{Cl}_2 (g) \rightarrow 2 \text{NOCl} (g) \]The general form of the rate law would be:\[ \text{Rate} = k \left[ \text{NO} \right]^m \left[ \text{Cl}_2 \right]^n \]#### Determining the Rate Law:To determine the rate law, compare the trials where only one reactant concentration changes while the other remains constant.- **Comparing trials 1 and 2 (change in [NO]):**\[\text{Rate}_2 / \text{Rate}_1 = \left( 4.0×10^{-2} \, \text{M/s} \right) / \left( 1.0×10^{-2} \, \text{M/s} \right)

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The initial rates listed in the following table were determined for the reaction: 2 NO (g) + Cl2 (g) → 2 NOCI (g) Initial Rate of Consumption of Cl2 Trial Initial [NO], (M) Initial [Cl2], (M) (M/s) 1 0.13 0.20 1.0x10-2 0.26 0.20 4.0x10-2 3 0.13 0.10 5.0x10-3 a. What is the rate law? b. What is the value of the rate constant, k? C. What is the initial rate when the initial concentrations of both reactants are 0.12 M?

The initial rates listed in the following table were determined for the reaction: 2 NO (g) + Cl2 (g) → 2 NOCI (g) Initial Rate of Consumption of Cl2 Trial Initial [NO], (M) Initial [Cl2], (M) (M/s) 1 0.13 0.20 1.0x10-2 0.26 0.20 4.0x10-2 3 0.13 0.10 5.0x10-3 a. What is the rate law? b. What is the value of the rate constant, k? C. What is the initial rate when the initial concentrations of both reactants are 0.12 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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