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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

The data in the table are for the reaction of NO and O2 at 660 K.

NO(g) + ½ O2(g) → NO2(g)

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  1. (a) Determine the order of the reaction for each reactant.
  2. (b) Write the rate equation for the reaction.
  3. (c) Calculate the rate constant.
  4. (d) Calculate the rate (in mol/L · s) at the instant when [NO] = 0.015 mol/L and [O2] = 0.0050 mol/L.
  5. (e) At the instant when NO is reacting at the rate 1.0 × 10−4 mol/L · s, what is the rate at which O2 is reacting and NO2 is forming?

(a)

Interpretation Introduction

Interpretation:

The order of the reaction for each reactant has to be determined

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]n

Order of a reaction: The order of a reaction with respect to a particular reactant is the exponent of its concentration term in the rate law expression, and the overall reaction order is the sum of the exponents on all concentration terms.

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

Explanation

The reaction rate of the chemical reaction is given as,

  Reaction Rate = k [NO]m[O2]n,where m, and n are orders of the reactants.Givenreaction: NO(g)+ 1/2 O2(g)NO2(g)Findorderofthereaction:_Comparingfirsttwoexperiments1and2,rate1=[NO]m[O2]n, rate1 = 2.5×10-5mol/L.srate2 = k [NO]m[O2]n, rate2 = 1.0×10-4mol/L.srate2rate1=k [NO]m[O2]nk [NO]m[O2]n1.0×10-4mol/L.s2.5×10-5mol/L.s=(0.020)m(0.010)n(0.010)m(0

(b)

Interpretation Introduction

Interpretation:

The rate equation for the reaction has to be written.

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]n

Order of a reaction: The order of a reaction with respect to a particular reactant is the exponent of its concentration term in the rate law expression, and the overall reaction order is the sum of the exponents on all concentration terms.

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

(c)

Interpretation Introduction

Interpretation:

The rate constant has to be calculated.

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]n

Order of a reaction: The order of a reaction with respect to a particular reactant is the exponent of its concentration term in the rate law expression, and the overall reaction order is the sum of the exponents on all concentration terms.

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

(d)

Interpretation Introduction

Interpretation:

The rate in (mol/L.s) has to be calculated.

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]n

Order of a reaction: The order of a reaction with respect to a particular reactant is the exponent of its concentration term in the rate law expression, and the overall reaction order is the sum of the exponents on all concentration terms.

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

(e)

Interpretation Introduction

Interpretation:

The rate at which O2 reacts and NO2 forms has to be given.

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]n

Order of a reaction: The order of a reaction with respect to a particular reactant is the exponent of its concentration term in the rate law expression, and the overall reaction order is the sum of the exponents on all concentration terms.

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

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