Please help with Part B Part A: In the hydrogenation of ethylene using a nickel catalyst, the initial concentration of ethylene is 1.80 mol⋅L−1mol⋅L−1 and its rate constant (kk) is 0.0015 mol⋅L−1⋅s−1mol⋅L−1⋅s−1 . Determine the rate of reaction if it follows a zero-order reaction mechanism.Answer: 1.5×10−3 mol⋅L−1⋅s−1mol⋅L−1⋅s−1Part B: The half-life of a reaction, t1/2t1/2t_{1/2}, 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 1.80 mol⋅L−1mol⋅L−1 and the rate constant is 0.0015 mol⋅L−1⋅s−1mol⋅L−1⋅s−1 . Learning Goal:To understand zero-order reactions.Chemical kinetics is the study of the speed withwhich a chemical reaction occurs and the factorsthat affect this speed. The speed of a reaction is therate at which the concentrations of reactants andproducts change. This relationship is expressedthrough rate laws.For a general reaction a A + bB gG+hH,the rate law is given asrate of reaction =k[A]™[B]"where the coefficients m and n are experimentallydetermined while a, b, g, and h are stoichiometriccoefficients unrelated to m and n.A zero-order reaction has a rate law in which thesum of the exponents m +n+...is equal tozero. Thus, if there is only one reactant, the rate ofreaction is independent of the concentration of thereactant.For a zero-order reaction, the graph of reactantconcentration versus time is a straight line.Therefore, the rate-law equation for a zero-orderreaction can be compared to that of a straight line,y = mx +6.

A numerical problem based on half-life period of zero order reaction, which is to be accomplished.

Answered: Please help with Part B Part A: In…

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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Please help with Part B

Part A: In the hydrogenation of ethylene using a nickel catalyst, the initial concentration of ethylene is 1.80 mol⋅L−1mol⋅L−1 and its rate constant (kk) is 0.0015 mol⋅L−1⋅s−1mol⋅L−1⋅s−1 . Determine the rate of reaction if it follows a zero-order reaction mechanism.

Answer: 1.5×10⁻³ mol⋅L−1⋅s−1mol⋅L−1⋅s−1

Part B: The half-life of a reaction, t1/2t1/2t_{1/2}, 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 1.80 mol⋅L−1mol⋅L−1 and the rate constant is 0.0015 mol⋅L−1⋅s−1mol⋅L−1⋅s−1 .

Learning Goal:
To understand zero-order reactions.
Chemical kinetics is the study of the speed with
which a chemical reaction occurs and the factors
that affect this speed. The speed of a reaction is the
rate at which the concentrations of reactants and
products change. This relationship is expressed
through rate laws.
For a general reaction a A + bB gG+hH,
the rate law is given as
rate of reaction =
k[A]™[B]"
where the coefficients m and n are experimentally
determined while a, b, g, and h are stoichiometric
coefficients unrelated to m and n.
A zero-order reaction has a rate law in which the
sum of the exponents m +n+...is equal to
zero. Thus, if there is only one reactant, the rate of
reaction is independent of the concentration 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 a straight line,
y = mx +6.

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