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Chemistry & Chemical Reactivity

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

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BuyFindarrow_forward

Chemistry & Chemical Reactivity

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

Data for the decomposition of dinitrogen monoxide

N2O(g) → N2(g) + ½ O2(g)

on a gold surface at 900 °C are given below. Verify that the reaction is first-order by preparing a graph of In[N2O] versus time. Derive the rate constant from the slope of the line in this graph. Using the rate law and value of k, determine the decomposition rate at 900 °C when [N2O] = 0.035 mol/L.

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Interpretation Introduction

Interpretation: The rate of decomposition at 900°C has to be given.

Concept Introduction:

The rate of reaction is the quantity of formation of product or the quantity of reactant used per unit time.  The rate of reaction doesn’t depend on the sum of amount of reaction mixture used.

The raise in molar concentration of product of a reaction per unit time or decrease in molarity of reactant per unit time is called rate of reaction and is expressed in units of mol/(L.s).

Integrated rate law for first order reaction:

Consider A as substance, that gives the product based on the equation,

    aAproducts

Where a= stoichiometric co-efficient of reactant A.

Consider the reaction has first-order rate law,

    Rate=-Δ[A]Δt=k[A]

The integrated rate law equation can be given as,

    ln[A]t[A]o=-kt

The above expression is called integrated rate law for first order reaction.

Explanation

The reaction rate of the chemical reaction is calculated as,

  Given:Time(min)ln[N2O](mol/L)15.02.48330.02.68880.03.352120.03.816Findthe slope for any two values:slope=Δln[N2O]Δt=2.688(2.482)3015=0.20515=0.0136k=slope=0.0136min1Therefore,[N2O]=0

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