Chemistry: The Molecular Nature of Matter and Change - Standalone book
Chemistry: The Molecular Nature of Matter and Change - Standalone book
7th Edition
ISBN: 9780073511177
Author: Martin Silberberg Dr., Patricia Amateis Professor
Publisher: McGraw-Hill Education
bartleby

Videos

Question
Book Icon
Chapter 17, Problem 17.109P

(a)

Interpretation Introduction

Interpretation:

The Kc for the system at temperature 900o C has to be calculated.

Concept Introduction:

Equilibrium constant:

The relationship between the concentration of products and concentration of reactants in a chemical reaction at equilibrium is said to be equilibrium constant.  It is denoted by K.

For a reaction,

  xX + yY  zZ

The expression of K can be given as

  Kc = [Z]z[X]x[Y]ywhere, [X] = equilibrium concentration of X [Y] = equilibrium concentration of Y [Z] = equilibrium concentration of Z

(a)

Expert Solution
Check Mark

Explanation of Solution

The reaction for the given system will be:

    CO(g) + H2O(g)  CO2(g) + H2(g)

Initial [CO] and initial [H2O] = 0.100mol/20.00L = 0.00500M

                          CO            H2O                 CO2          H2Initial              0.00500M    0.00500M                     0                0Change               -x                 -x                              +x              +x-----------------------------------------------------------------------------------Equilibrium   0.00500-x     0.00500-x                       x                x   [CO]equlibrium=  0.00500-x  =  2.24×10-3M  =  [H2O]         x = 0.00276 M = [CO2] = [H2]         Kc[CO2][H2][CO][H2O] = [0.00276][0.00276][0.00224][0.00224] = 1.518176 = 1.52

(b)

Interpretation Introduction

Interpretation:

Ptotal in the flask at equilibrium has to be calculated.

(b)

Expert Solution
Check Mark

Explanation of Solution

The reaction for the given system will be:

    CO(g) + H2O(g)  CO2(g) + H2(g)

    Mtotal= [CO] + [H2O] + [CO2] + [H2]               = (0.00224 M) + (0.00224 M) + (0.00276 M) + (0.00276 M)              = 0.01000 MMntotal = (Mtotal)(V) = (0.01000 mol/L)(20.00L) = 0.2000 mol totalPV = nRT (ideal gas equation)Ptotal= ntotalRT/V = (0.2000mol)(0.0806LatmmolK)((273+900)K)(20.00L)      = 0.9625638 = 0.9626atm

(c)

Interpretation Introduction

Interpretation:

The number of moles that must be added to double pressure has to be found.

(c)

Expert Solution
Check Mark

Explanation of Solution

According to ideal gas equation PV = nRT

Pressure is directly proportional to number of moles.

Then equal number of moles must be added = 0.2000 mol CO

(d)

Interpretation Introduction

Interpretation:

After Ptotal is doubled and the system remains equilibrium, [CO]eq has to be found.

Concept Introduction:

Equilibrium constant:

The relationship between the concentration of products and concentration of reactants in a chemical reaction at equilibrium is said to be equilibrium constant.  It is denoted by K.

For a reaction,

  xX + yY  zZ

The expression of K can be given as

  Kc = [Z]z[X]x[Y]ywhere, [X] = equilibrium concentration of X [Y] = equilibrium concentration of Y [Z] = equilibrium concentration of Z

(d)

Expert Solution
Check Mark

Explanation of Solution

The reaction for the given system will be:

    CO(g) + H2O(g)  CO2(g) + H2(g)

  Initial [CO] and initial [H2O] = 0.100mol/20.00L = 0.00500MTo that add 0.2000molCO/20.00L = 0.01000 M to compensate for the added CO

                            CO            H2O                 CO2          H2Initial              0.00224 M    0.00224M                0.00276 M   0.00276 MAdded CO       0.01000 M   Change               -x                 -x                              +x              +x-----------------------------------------------------------------------------------Equilibrium   0.01224-x     0.00224-x                0.00276+x   0.00276+x            Kc[CO2][H2][CO][H2O] = [0.00276+x][0.00276+x][0.01224-x][0.00224-x] = 1.518176                        [7.6176×10-6+5.52×10-3x+x2][2.7417×10-5-1.448×10-2x+x2] = 1.518176       7.6176×10-6+5.52×10-3x+x2= (1.518176)(2.7417×10-5-1.448×10-2x+x2)       0.51817x2-0.027503x + 3.400714×10-5= 0a = 0.518176 , b = -0.027503 , c = 3.400714×10-5x = -b±b2-4ac2ax = -(-0.027503) ± (-0.027503)2-4(0.518176)(3.400714×10-5)2(0.518176)x = 1.31277×10-3[CO] = 0.01224-x = 0.01224-(1.31277×10-3) = 0.01092723 = 0.01093 M

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Chapter 17 Solutions

Chemistry: The Molecular Nature of Matter and Change - Standalone book

Ch. 17.5 - Prob. 17.6AFPCh. 17.5 - Prob. 17.6BFPCh. 17.5 - Prob. 17.7AFPCh. 17.5 - Prob. 17.7BFPCh. 17.5 - Prob. 17.8AFPCh. 17.5 - Prob. 17.8BFPCh. 17.5 - Prob. 17.9AFPCh. 17.5 - Prob. 17.9BFPCh. 17.5 - Prob. 17.10AFPCh. 17.5 - Prob. 17.10BFPCh. 17.5 - An inorganic chemist studying the reactions of...Ch. 17.5 - A chemist studying the production of nitrogen...Ch. 17.6 - In a study of glass etching, a chemist examines...Ch. 17.6 - Prob. 17.12BFPCh. 17.6 - Prob. 17.13AFPCh. 17.6 - Prob. 17.13BFPCh. 17.6 - Prob. 17.14AFPCh. 17.6 - Should T be increased or decreased to yield more...Ch. 17.6 - Prob. 17.15AFPCh. 17.6 - Prob. 17.15BFPCh. 17.6 - Many metabolites are products in branched...Ch. 17 - Prob. 17.1PCh. 17 - When a chemical company employs a new reaction to...Ch. 17 - If there is no change in concentrations, why is...Ch. 17 - Prob. 17.4PCh. 17 - Prob. 17.5PCh. 17 - Prob. 17.6PCh. 17 - Prob. 17.7PCh. 17 - Prob. 17.8PCh. 17 - Prob. 17.9PCh. 17 - Does Q for the formation of 1 mol of NO from its...Ch. 17 - Does Q for the formation of 1 mol of NH3 from H2...Ch. 17 - Balance each reaction and write its reaction...Ch. 17 - Prob. 17.13PCh. 17 - Prob. 17.14PCh. 17 - Prob. 17.15PCh. 17 - At a particular temperature, Kc = 1.6×10−2...Ch. 17 - Prob. 17.17PCh. 17 - Balance each of the following examples of...Ch. 17 - Balance each of the following examples of...Ch. 17 - Balance each of the following examples of...Ch. 17 - Balance each of the following examples of...Ch. 17 - Prob. 17.22PCh. 17 - Prob. 17.23PCh. 17 - Prob. 17.24PCh. 17 - When are Kc and Kp equal, and when are they not? Ch. 17 - A certain reaction at equilibrium has more moles...Ch. 17 - Prob. 17.27PCh. 17 - Determine Δngas for each of the following...Ch. 17 - Prob. 17.29PCh. 17 - Prob. 17.30PCh. 17 - Prob. 17.31PCh. 17 - Prob. 17.32PCh. 17 - Prob. 17.33PCh. 17 - The following molecular scenes depict the aqueous...Ch. 17 - At 425°C, Kp = 4.18 × 10−9 for the...Ch. 17 - At 100°C, Kp = 60.6 for the reaction 2NOBr(g) ⇌...Ch. 17 - The water-gas shift reaction plays a central role...Ch. 17 - In the 1980s, CFC-11 was one of the most heavily...Ch. 17 - For a problem involving the catalyzed reaction of...Ch. 17 - What is the basis of the approximation that avoids...Ch. 17 - Prob. 17.41PCh. 17 - Gaseous ammonia was introduced into a sealed...Ch. 17 - Prob. 17.43PCh. 17 - Prob. 17.44PCh. 17 - Prob. 17.45PCh. 17 - Prob. 17.46PCh. 17 - Prob. 17.47PCh. 17 - Prob. 17.48PCh. 17 - Prob. 17.49PCh. 17 - Nitrogen dioxide decomposes according to the...Ch. 17 - Hydrogen iodide decomposes according to the...Ch. 17 - Compound A decomposes according to the...Ch. 17 - In an analysis of interhalogen reactivity, 0.500...Ch. 17 - A toxicologist studying mustard gas, S(CH2CH2Cl)2,...Ch. 17 - Prob. 17.55PCh. 17 - A key step in the extraction of iron from its ore...Ch. 17 - What does “disturbance” mean in Le Châtelier’s...Ch. 17 - Prob. 17.58PCh. 17 - Prob. 17.59PCh. 17 - Prob. 17.60PCh. 17 - Le Châtelier’s principle is related ultimately to...Ch. 17 - An equilibrium mixture of two solids and a gas, in...Ch. 17 - Consider this equilibrium system: CO(g) + Fe3O4(s)...Ch. 17 - Sodium bicarbonate undergoes thermal decomposition...Ch. 17 - Prob. 17.65PCh. 17 - Prob. 17.66PCh. 17 - Predict the effect of decreasing the container...Ch. 17 - Prob. 17.68PCh. 17 - Prob. 17.69PCh. 17 - Prob. 17.70PCh. 17 - Prob. 17.71PCh. 17 - Prob. 17.72PCh. 17 - Prob. 17.73PCh. 17 - The formation of methanol is important to the...Ch. 17 - Prob. 17.75PCh. 17 - The oxidation of SO2 is the key step in H2SO4...Ch. 17 - A mixture of 3.00 volumes of H2 and 1.00 volume of...Ch. 17 - You are a member of a research team of chemists...Ch. 17 - For the following equilibrium system, which of the...Ch. 17 - Prob. 17.80PCh. 17 - Prob. 17.81PCh. 17 - Prob. 17.82PCh. 17 - Prob. 17.83PCh. 17 - Prob. 17.84PCh. 17 - Prob. 17.85PCh. 17 - Prob. 17.86PCh. 17 - Prob. 17.87PCh. 17 - Prob. 17.88PCh. 17 - When 0.100 mol of CaCO3(s) and 0.100 mol of CaO(s)...Ch. 17 - Prob. 17.90PCh. 17 - Prob. 17.91PCh. 17 - Prob. 17.92PCh. 17 - Highly toxic disulfur decafluoride decomposes by a...Ch. 17 - A study of the water-gas shift reaction (see...Ch. 17 - Prob. 17.95PCh. 17 - Prob. 17.96PCh. 17 - Prob. 17.97PCh. 17 - Prob. 17.98PCh. 17 - Prob. 17.99PCh. 17 - Prob. 17.100PCh. 17 - The molecular scenes below depict the reaction Y ⇌...Ch. 17 - For the equilibrium H2S(g) ⇌ 2H2(g) + S2(g) Kc =...Ch. 17 - Prob. 17.103PCh. 17 - Prob. 17.104PCh. 17 - The kinetics and equilibrium of the decomposition...Ch. 17 - Isopentyl alcohol reacts with pure acetic acid to...Ch. 17 - Isomers Q (blue) and R (yellow) interconvert. They...Ch. 17 - Glauber’s salt, Na2SO4·10H2O, was used by J. R....Ch. 17 - Prob. 17.109PCh. 17 - Synthetic diamonds are made under conditions of...
Knowledge Booster
Background pattern image
Chemistry
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Recommended textbooks for you
Text book image
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Text book image
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Text book image
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Text book image
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Text book image
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Text book image
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY
Chemical Equilibria and Reaction Quotients; Author: Professor Dave Explains;https://www.youtube.com/watch?v=1GiZzCzmO5Q;License: Standard YouTube License, CC-BY