Chapter 14, Problem 12PS

### Chemistry & Chemical Reactivity

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

Chapter
Section

### Chemistry & Chemical Reactivity

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

# The reaction2 NO(g) + 2 H2(g) → N2(g) + 2 H2O(g)was studied at 904 °C, and the data in the table were collected. (a) Determine the order of the reaction for each reactant. (b) Write the rate equation for the reaction. (c) Calculate the rate constant for the reaction. (d) Find the rate of appearance of N2 at the instant when [NO] = 0.350 mol/L and [H] = 0.205 mol/L.

(a)

Interpretation Introduction

Interpretation: The order of the reaction for each reactant 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.

Explanation

The order of the reaction is calculated as,

â€‚Â ReactionÂ Rateâ€‰Â =Â kÂ [NO]m[H2]n,whereÂ m,Â andÂ nÂ areÂ ordersÂ ofÂ theÂ reactants.Givenâ€‰reaction:Â 2Â NOâ€‰(g)Â +Â 2Â H2(g)Â®N2(g)â€‰+Â 2Â H2OÂ (g)Findâ€‰orderâ€‰ofâ€‰theâ€‰reaction:_Comparingâ€‰firstâ€‰twoâ€‰experimentsâ€‰1â€‰andâ€‰2,rateâ€‰1=â€‰kÂ [NO]m[H2]n,Â rate1Â =Â 0.136Â mol/L.srateâ€‰2Â =Â kÂ [NO]m[H2]n,Â rate2Â =Â 0.0339Â mol/L.srate1rateâ€‰2=kÂ [NO]m[H2]nkÂ [NO]m[H2]n0.136mol/L.s0.0339mol/L.s=(0.420)m(0.122)n(0.210)m(0

(b)

Interpretation Introduction

Interpretation: The rate of 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 order of the reaction for each reactant 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 of appearance of N2 at the instant has to be found.

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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