Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074



Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

For the reaction C2F4 → ½ C4F8, a graph of 1/[C2F4] versus time gives a straight line with a slope of + 0.04 L/mol · s. What is the rate law for this reaction?

Interpretation Introduction


For the given reaction under given reaction conditions that is with given slope value as +0.04L/mol.s the rate law for the given chemical equation should be determined.

Concept introduction:

In order to establish the plausibility of a mechanism, one must compare the rate law of the rate determining step to the experimentally determined rate law.

Rate determining step: In a chemical reaction the rate determining step is the slowest step in which the rate of the reaction depends on the rate of that slowest step.

Rate law: It is generally the rate equation that consists of the reaction rate with the concentration or the pressures of the reactants and constant parameters.

Activation energy: It is defined as the minimum energy required by the reacting species in order to undergo chemical reaction.

Rate constant: The rate constant for a chemical reaction is the proportionality term in the chemical reaction rate law which gives the relationship between the rate and the concentration of the reactant present in the chemical reaction.

Intermediate species: It is the species formed during the middle of the chemical reaction between the reactant and the desired product.



The slope plotted versus 1C2F4 with time gives straight line with slope value equal to +0.04L/mol.s.

The given chemical reaction is as follows,


The rate law of a chemical reaction is an expression that relates the concentration of the reactant with the rate.

The rate law contains proportionality term and the concentration of reactants which their coefficient are raised to the power.  Here, it is given that the plotted graph is a straight line which says that the given reaction is second order

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