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

Gaseous NO2 decomposes at 573 K.

NO2(g) → NO(g) + ½ O2(g)

The concentration of NO2 was measured as a function of time. A graph of 1/[NO2] versus time gives a straight line with a slope of 1.1 L/mol · s. What is the rate law for this reaction? What is the rate constant?

Interpretation Introduction


The rate law and rate constant has to be given.

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.

Arrhenius equation:

  • Arrhenius equation is a formula that represents the temperature dependence of reaction rates
  • The Arrhenius equation has to be represented as follows


  • Ea represents the activation energy and it’s unit is kJ/mol
  • R represents the universal gas constant and it has the value of 8.314 J/K.mol
  • T represents the absolute temperature
  • A represents the frequency factor or collision frequency
  • e represents the base of natural logarithm
  •  Arrhenius equation equation was proposed by Svante Arrhenius in 1889.

The slope plotted versus 1NO2 with time gives straight line with slope value equal to 1.1L/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

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