### Zero-Order Reactions**Learning Goal:** To understand zero-order reactions.Chemical kinetics studies the speed of chemical reactions and their influencing factors. The speed of a reaction is the rate of change in concentrations of reactants and products, expressed through rate laws.For a general reaction:\[ aA + bB \rightarrow gG + hH \]The rate law is:\[ \text{rate of reaction} = k[A]^m[B]^n \]where the coefficients \(m\) and \(n\) are experimentally determined, while \(a, b, g, h\) are stoichiometric coefficients unrelated to \(m\) and \(n\).A zero-order reaction has a rate law where the sum \(m + n + \ldots = 0\). Thus, if there's one reactant, the rate is independent of its concentration.In zero-order reactions, the concentration versus time graph is a straight line. The rate-law equation is analogous to a straight line equation \(y = mx + b\).**Exercise:**- **Multiple Choice:** - The units for the rate constant and reaction rate are the same - Zero-order reactions slow down as they proceed - Reactant concentration changes nonlinearly - Reaction rate does not equal the rate constant - Higher reactant concentration does not increase rate**Correct Answer:**- A zero-order reaction is independent of reactant concentration. Features include: 1. Concentration vs. time graph is a straight line with a negative slope equal to the rate constant. 2. The rate of reaction equals the rate constant. 3. Units: \([L \cdot mol^{-1} \cdot s^{-1}]\).**Examples:** Photochemical and surface reactions.**Part B:**In the hydrogenation of ethylene using a nickel catalyst, initial ethylene concentration is \(1.50 \, \text{mol} \cdot \text{L}^{-1}\), and \(k = 0.0012 \, \text{mol} \cdot \text{L}^{-1} \cdot \text{s}^{-1}\). Calculate the reaction rate assuming a zero-order mechanism, expressed to two significant figures with appropriate units.- **Incorrect Attempt:** - Rate = 541.6 \(\text{mol/L}\) (Try again

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In the hydrogenation of ethylene using a nickel catalyst, the initial concentration of ethylene is 1.50 mol-L. and its rate constant (k) is 0.0012 mol-L-Determine the rate of reaction if it follows a zero- order reaction mechanism.

In the hydrogenation of ethylene using a nickel catalyst, the initial concentration of ethylene is 1.50 mol-L. and its rate constant (k) is 0.0012 mol-L-Determine the rate of reaction if it follows a zero- order reaction mechanism.

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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