   Chapter 14, Problem 8PS

Chapter
Section
Textbook Problem

A reaction has the experimental rate equation Rate = k[A]2. How will the rate change if the concentration of A is tripled? If the concentration of A is halved?

Interpretation Introduction

Interpretation: The rate change at the given conditions has to be explained.

Concept introduction:

Rate law or rate equation: The relationship between the reactant concentrations and reaction rate is expressed by an equation.

aA + bBxXRate of reaction = k [A]m[B]nTotalorderof reaction = (m + n)

Rate constant, k: It is a proportionality constant that relates rate and concentration at a given temperature.

Explanation

Reaction Rate = k [A]n,where n is the order of the reactant.Givenreaction rate : Rate = k [A]2Orderoftheoverallreaction:_ Condition 1: Concentration of A is tripled as (3A),thenRate

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