Chemistry: Atoms First
Chemistry: Atoms First
3rd Edition
ISBN: 9781259638138
Author: Julia Burdge, Jason Overby Professor
Publisher: McGraw-Hill Education
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Chapter 15, Problem 15.145QP

The equilibrium constant Kc for the reaction

2NH 3 ( g ) N 2 ( g ) + 3H 2 ( g )

is 0.83 at 375°C. A 14.6-g sample of ammonia is placed in a 4.00-L flask and heated to 375°C. Calculate the concentrations of all the gases when equilibrium is reached.

Expert Solution & Answer
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Interpretation Introduction

Interpretation:

To calculate the equilibrium concentration values are given homogenies equilibrium of ammonia (NH3) dissociation reaction with respective pressure and temperature at 375οC .

Concept Introduction:

Equilibrium concentration: If Kc and the initial concentration for a reaction and calculate for both equilibrium concentration, and using the (ICE) chart and equilibrium constant and derived changes in respective reactants and products.

Pressure effect in equilibrium: The equilibrium constant calculated from the partial pressures of a reaction equation. It is used to express the relationship between product pressures and reactant pressures. It is unites number, although it relates the pressures.

Homogeneous equilibrium: A homogeneous equilibrium involved has a everything present in the same phase and same conditions, for example reactions where everything is a gas, or everything is present in the same solution.

Temperature affect in equilibrium: This process chemical shifts changes (or) towards the product or reactant, which can be determined by studying the reaction and deciding whether it is exothermic or endothermic.

Le Chatelier's Principle (Kp): The closed system is an increase in pressure, the equilibrium will shift towards the sides of the reaction with some moles of gas. The decrease in pressure the equilibrium will shift towards the side of the reaction with high moles of gas.

Answer to Problem 15.145QP

The reactant and product each equilibrium concentration (ICE) values for the given NH3 ammonia dissociation reaction is shown below.

2NH3(g)N2(g)+3H2(g)Kc=[N2][H2]3[NH3]2[NH3]=0.042M,[N2]=0.086Mand[H2]=0.26M

Explanation of Solution

To find: The equilibrium concentration should be identified given the gases phase reaction.

Analyze the chemical equilibrium reaction.

N2(g)+3H2(g)2NH3(g)[FormationReaction]2NH3(g)N2(g)+3H2(g)---------[Decomposition Reaction]

Given the gas phase equilibrium concentration reaction is the combined reaction; it is the product of the constants for this component reaction. This equilibrium reaction expression contains same conditions like gas phase. Hence this process homogenous equilibrium further the equilibrium constant can also be represented by Kc, were the Kp represents partial pressure. Then the each (reactant and product) molecule equilibrium concentration (N2, H2and NH3) are discussed and explained the fallowing below method.

To find: Calculate the each concentration values for given the equilibrium constant (Kc) of ammonia dissociation reaction.

Calculate and analyze the respective concentration values at 3750C .

First let’s calculate the initial concentration of ammonia.

[NH3]=14.6g×1molofNH317.03gofNH34.00L[MolarMassofNH3=17.03g]=14.6g×0.058714.00L=0.85714.00L=0.214Theconcentrationof[NH3]=0.214M

Further we set up a ICE table to represent the equilibrium concentrations. With respect the amount of (NH3) that reacts as (2x) fallowed by,

2NH3(g)N2(g)+3H2(g)Initial (M): 0.21400Change (M):  -2x+x+3xEqilibrium (M):(0.2142x)x3xSubstituteintothe equilibriumexpressiontosolvefor(x).Kc=[N2][H2]3[NH3]2Therespactive equilbriumconcentrationvaluesareN2=+x,H2=3xandNH3=0.2142xThepartialpresurevaluesof(NH3)=0.83The respactive values are substituted equation (1)0.83=(x)(3x)2(0.2142x)2=27x4(0.2142x)2[2]Takingthe square rootof both sidesof theaboveequation(2)0.91=5.20x20.2142x[3]Rearrangingequation(3)5.20x2+1.82x0.195=0Solvingthequadraticequationgivestheaboveequationx=b±b24ac2ax=0.086Mandx=0.44MHerethe possitiverootandequilibriumconcetrationsareNH3=0.2142x(x=0.086M)[NH3]=0.2142(0.086)=0.0442M[N2]=0.086MH2=3x;3(0.086)=0.26M

The given ammonia dissociation reaction the respective reactant to give a two moles of products, and this reaction proceeds in same phase  and this equilibrium reaction expression contains single conditions like gases phase, the equilibrium constant can also be represented by Kp, were the “P” partial pressure. The each reactant and product concentration values are derived given above equation at 3750C finally the equilibrium constant of following methods as showed above.

Conclusion

The each of reactant and product equilibrium concentration values are derived given the gas phase ammonia (NH3) dissociation equilibrium reactions.

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Chapter 15 Solutions

Chemistry: Atoms First

Ch. 15.3 - Write equilibrium expressions for each of the...Ch. 15.3 - Write equilibrium expressions for each of the...Ch. 15.3 - Which of the following equilibrium expressions...Ch. 15.3 - Consider the reaction A(s)+B(g)C(s). 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The diagram shown on...Ch. 15.4 - The equilibrium constant, KP, for the reaction...Ch. 15.4 - G for the reaction H2(g)+I2(s)2HI(g) is 2.60...Ch. 15.4 - Prob. 8PPBCh. 15.4 - Prob. 8PPCCh. 15.4 - Using data from Appendix 2, calculate the...Ch. 15.4 - Prob. 9PPACh. 15.4 - Kf for the complex ion Ag(NH3)2+ is 1.5 107 at...Ch. 15.4 - Which of the following graphs [(i)(iv)] best shows...Ch. 15.4 - The equilibrium constant, Ksp, for the dissolution...Ch. 15.4 - Calculate G for the process:...Ch. 15.4 - Ksp for Co(OH)2 at 25C is 3.3 10-16 Using this and...Ch. 15.4 - Prob. 10PPCCh. 15.4 - Free Energy and Chemical Equilibrium 15.4.1 For...Ch. 15.4 - The Ksp for iron(III) hydroxide [Fe(OH)3] is 1.1 ...Ch. 15.4 - Prob. 15.4.3SRCh. 15.5 - Kc for the reaction of hydrogen and iodine to...Ch. 15.5 - Calculate the equilibrium concentrations of H2,...Ch. 15.5 - Determine the initial concentration of HI if the...Ch. 15.5 - Consider the reaction A(g) + B(g) C(g). The...Ch. 15.5 - For the same reaction and temperature as in Worked...Ch. 15.5 - Prob. 12PPACh. 15.5 - Prob. 12PPBCh. 15.5 - Prob. 12PPCCh. 15.5 - At elevated temperatures, iodine molecules break...Ch. 15.5 - Aqueous hydrocyanic acid (HCN) ionizes according...Ch. 15.5 - Consider a weak acid, HA, that ionizes according...Ch. 15.5 - Prob. 13PPCCh. 15.5 - A mixture of 5.75 atm of H2 and 5.75 atm of I2 is...Ch. 15.5 - Prob. 14PPACh. 15.5 - Prob. 14PPBCh. 15.5 - Consider the reaction A(g)+B(g)C(s)+D(s). The...Ch. 15.5 - Define equilibrium. Give two examples of a dynamic...Ch. 15.5 - Prob. 15.5.2SRCh. 15.5 - Prob. 15.5.3SRCh. 15.6 - Hydrogen sulfide (H2S) is a contaminant commonly...Ch. 15.6 - For each change indicated, determine whether the...Ch. 15.6 - What can be added to the equilibrium that will (a)...Ch. 15.6 - Consider the reaction A(g)+B(g)C(s)+D(s), of the...Ch. 15.6 - For each reaction, predict in what direction the...Ch. 15.6 - For each reaction, predict the direction of shift...Ch. 15.6 - For the following equilibrium, give an example of...Ch. 15.6 - Prob. 16PPCCh. 15.6 - Factors That Affect Chemical Equilibrium 15.6.1...Ch. 15.6 - Indicate in which direction the following...Ch. 15.6 - Prob. 15.6.3SRCh. 15.6 - The diagrams show equilibrium mixtures of A2, B2,...Ch. 15 - The Ka for hydrocyanic acid (HCN) is 4.9 10 l0....Ch. 15 - Determine the concentrations of Pb2+ and I in a...Ch. 15 - Determine the Ka for a weak acid if a 0.10-M...Ch. 15 - Prob. 15.4KSPCh. 15 - Define equilibrium. Give two examples of a dynamic...Ch. 15 - Which of the following statements is collect about...Ch. 15 - Consider the reversible reaction A B. Explain how...Ch. 15 - What is the law of mass action?Ch. 15 - Briefly describe the importance of equilibrium in...Ch. 15 - Define reaction quotient. How does it differ from...Ch. 15 - Prob. 15.7QPCh. 15 - Write the equation for the reaction that...Ch. 15 - Prob. 15.9QPCh. 15 - The equilibrium constant for the reaction...Ch. 15 - Prob. 15.11QPCh. 15 - The equilibrium constant for the reaction...Ch. 15 - Prob. 15.13QPCh. 15 - Prob. 15.14QPCh. 15 - Prob. 15.15QPCh. 15 - Prob. 15.16QPCh. 15 - Prob. 15.17QPCh. 15 - Write equilibrium constant expressions for Kc and...Ch. 15 - Write the equilibrium constant expressions for Kc...Ch. 15 - Prob. 15.20QPCh. 15 - Prob. 15.21QPCh. 15 - Prob. 15.22QPCh. 15 - Computational Problems 15.23 The equilibrium...Ch. 15 - Prob. 15.24QPCh. 15 - The equilibrium constant KP for the reaction is...Ch. 15 - Prob. 15.26QPCh. 15 - Prob. 15.27QPCh. 15 - Prob. 15.28QPCh. 15 - Prob. 15.29QPCh. 15 - The equilibrium constant Kp for foe reaction is...Ch. 15 - Ammonium carbamate (NH4CO2NH2) decomposes as...Ch. 15 - Prob. 15.32QPCh. 15 - Consider the equilibrium If nitrosyl bromide...Ch. 15 - Prob. 15.34QPCh. 15 - The following equilibrium constants have been...Ch. 15 - 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Prob. 15.124QPCh. 15 - The equilibrium constant Kc for the following...Ch. 15 - The equilibrium constant (KP for the formation of...Ch. 15 - Prob. 15.127QPCh. 15 - Prob. 15.128QPCh. 15 - Prob. 15.129QPCh. 15 - In the gas phase, nitrogen dioxide is actually a...Ch. 15 - A 2.50-mole sample of NOCl was initially in a...Ch. 15 - About 75% of hydrogen for industrial use is...Ch. 15 - Photosynthesis can be represented by...Ch. 15 - Consider the decomposition of ammonium chloride at...Ch. 15 - At 25C, the equilibrium partial pressures of NO2...Ch. 15 - In 1899 the German chemist Ludwig Mond developed a...Ch. 15 - Consider the equilibrium reaction described in...Ch. 15 - Consider the equilibrium system3AB. Sketch the...Ch. 15 - The vapor pressure of mercury is 0.0020 mmHg at...Ch. 15 - Large quantities of hydrogen are needed for the...Ch. 15 - Prob. 15.141QPCh. 15 - At 25C. a mixture of NO2 and N2O4 gases are m...Ch. 15 - Prob. 15.143QPCh. 15 - Heating copper (II) oxide at 400C does not produce...Ch. 15 - The equilibrium constant Kc for the reaction...Ch. 15 - The dependence of the equilibrium constant of a...Ch. 15 - Prob. 15.147QPCh. 15 - The following diagram shows the variation of the...Ch. 15 - The Kp for the reaction SO2Cl2(g)SO2(g)+Cl2(g) is...Ch. 15 - Derive the equation G=RTlnQK where Q is the...Ch. 15 - Prob. 15.151QPCh. 15 - Prob. 15.152QPCh. 15 - Prob. 15.153QPCh. 15 - Industrial production of ammonia from hydrogen and...Ch. 15 - For which of the following reactions is Kc equal...Ch. 15 - At present, the World Anti-Doping Agency has no...Ch. 15 - (a) Use the vant Hoff equation in Problem 15.146...
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