   # The reaction 2 NO(g) + 2 H 2 (g) → N 2 (g) + 2 H 2 O(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 N 2 at the instant when [NO] = 0.350 mol/L and [H] = 0.205 mol/L. ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 14, Problem 12PS
Textbook Problem
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## 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 of Solution

The order of the reaction is calculated as,

Reaction Rate = k [NO]m[H2]n,where m, and n are orders of the reactants.Givenreaction: 2 NO(g) + 2 H2(g)®N2(g)+ 2 H2(g)Findorderofthereaction:_Comparingfirsttwoexperiments1and2,rate1=[NO]m[H2]n, rate1 = 0.136 mol/L.srate2 = k [NO]m[H2]n, rate2 = 0.0339 mol/L.srate1rate2=k [NO]m[H2]nk [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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