Learning Goal:To understand zero-order reactions.Chemical kinetics is the study of the speed with which a chemical reaction occurs and thefactors that affect this speed. The speed of a reaction is the rate at which theconcentrations of reactants and products change. This relationship is expressed throughrate laws.For a general reaction aA + bBgG+ hH, the rate law is given asrate of reaction = k[A] [B]"where the coefficients and are experimentally determined while a, b, g, and h arestoichiometric coefficients unrelated to me and mAzero-order reaction has a rate law in which the sum of the exponents m+n+... isequal to zero. Thus, if there is only one reactant, the rate of reaction is independent of theconcentration of the reactant.For a zero-order reaction, the graph of reactant concentration versus time is a straight line.Therefore, the rate-law equation for a zero-order reaction can be compared to that of astraight line, y = mz+b.In the hydrogenation of ethylene using a nickel catalyst, the initial concentration of ethylene is 1.50 mol-L-¹ and its rate constant (k) is 0.0012 mol-Ls. Determine the rate of reaction if it follows a zero-order reaction mechanism.Express your answer to two significant figures and include the appropriate units.▸ View Available Hint(s)rate of reaction = 1.2x10-3 mol-L-¹-1Submit✓ CorrectPrevious AnswersIntegrated rate law for a zero-order reactionThe integrated rate law for a chemical reaction is a relationship between the concentrations of the reactants and time. Consider a single reactant A decomposing into products: A → products.For a zero-order reaction,Because the rate of the reaction is -A[A]/At, the above rate law can be written asOn integrating this differential equation, the integrated rate law for a zero-order reaction is obtained:▾ Part C[A] = -kt +[A]owhere [A], is the concentration at time t, le is the rate constant, and [A]o is the initial concentration. The variation in concentration with time provides a detailed description of how fast the reaction is occurring.Submitrate kThe half-life of a reaction, t₁/2, is the time required for one-half of a reactant to be consumed. It is the time during which the amount of reactant or its concentration decreases to one-half of its initial value.Determinethe half-life for the reaction in Part B using the integrated rate law, given that the initial concentration is 1.50 mol-L and the rate constant is 0.0012 mol-L-¹-s-¹.Express your answer to two significant figures and include the appropriate units.▸ View Available Hint(s)Templates Symbols undo redo Teset keyboard shortcuts helpUnitst1/2 = Value-A[A]At

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The half-life of a reaction, f/2. is the time required for one-half of a reactant to be consumed. It is the time during which the amount of reactant or its concentration decreases to one-half of its initial value Determine the half-life for the reaction in Part B using the integrated rate law, given that the initial concentration is 1.50 mol-L and the rate constant is 0.0012 mol-L-s Express your answer to two significant figures and include the appropriate units. ▸ View Available Hint(s)

The half-life of a reaction, f/2. is the time required for one-half of a reactant to be consumed. It is the time during which the amount of reactant or its concentration decreases to one-half of its initial value Determine the half-life for the reaction in Part B using the integrated rate law, given that the initial concentration is 1.50 mol-L and the rate constant is 0.0012 mol-L-s Express your answer to two significant figures and include the appropriate units. ▸ View Available Hint(s)

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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our is all about Chemical kinetics please help plsssss... please answer FIRST QUESTION ONLY