CHEMISTRY THE CENTRAL SCIENCE >EBOOK<
14th Edition
ISBN: 9780136873891
Author: Brown
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Videos
Textbook Question
Chapter 15, Problem 41E
a. If QC< KC, in which direction will a reaction proceed in order to reach equilibrium?
b. what condition must be satisfied so that Qc= KC?
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
(a) If Qc < Kc, in which direction will a reaction proceedin order to reach equilibrium? (b) What condition mustbe satisfied so that Qc = Kc?
1. (a) If Qc < Kc, in which direction will a reaction proceed in order to reach
equilibrium? (b) What condition must be satisfied so that Qc = Kc?
%3D
Ethyl acetate is synthesized in a nonreacting solvent (not water) according to the following reaction:
CH; CO,H+ C,HOH = CH3 CO2C,Hs +H20
K= 2.2
Acetic acid
Ethanol
Ethyl acetate
For the following mixtures (a-d), will the concentration of H20 increase, decrease, or remain the same as equilibrium is established?
a. [CH3 CO2C2H5] = 0.22 M, H20] = 0.10 M, [CH, CO,H] = 0.010M, [C,H;OH] = 0.010 M
increase
O decrease
O remain the same
b. [CH3CO2 C,H,] = 0.22 M, [H20] = 0.0020 M, [CH,CO,H] = 0.0020 M, [C2H, OH]= 0.10 M
Oincrease
O decrease
Oremain the same
c. [CH; CO,C, H5] = 0.88 M. (H,O] = 0.12 M. [CH,CO,H = 0.044 M, [C,H; OH] = 6.0 M
O increase
O decrease
O remain the same
d. [CH3 CO2C2 Hs] = 4.4 M, H20] = 4.4 M. [CH,CO,H = 0.88 M. [C2H;OH] = 10.0 M
O increase
decrease
Oremain the same
e. What must the concentration of water be for a mixture with [CH3CO,C,H;] = 1.0 M, [CH3CO,H = 0.10 M, and [C2H, OH] = 7.0 M to be
at equilibrium?
Concentration =
M
Chapter 15 Solutions
CHEMISTRY THE CENTRAL SCIENCE >EBOOK<
Ch. 15.2 - Prob. 15.1.1PECh. 15.2 - Prob. 15.1.2PECh. 15.2 - Prob. 15.2.1PECh. 15.2 - Prob. 15.2.2PECh. 15.3 - Prob. 15.3.1PECh. 15.3 - Practice Exercise 2 For the reaction H2 (g) + I2...Ch. 15.3 - Prob. 15.4.1PECh. 15.3 - Prob. 15.4.2PECh. 15.4 - Prob. 15.5.1PECh. 15.4 - Prob. 15.5.2PE
Ch. 15.4 - Practice Exercise 1
If 8.0 g of NH4HS(s)...Ch. 15.4 - Prob. 15.6.2PECh. 15.5 - Practice Exercise 1
A mixture of gaseous sulfur...Ch. 15.5 - Prob. 15.7.2PECh. 15.5 - Practice Exercise 1 In Section 15.1, we discussed...Ch. 15.5 - Practice Exercise 2
The gaseous compound BrCl...Ch. 15.6 - Prob. 15.9.1PECh. 15.6 - Practice Exercise 2 At 1000 k, the value of Kp for...Ch. 15.6 - Prob. 15.10.1PECh. 15.6 - Prob. 15.10.2PECh. 15.6 - Practice Exercise 1 For the equilibrium Br2(g) +...Ch. 15.6 - Prob. 15.11.2PECh. 15.7 - Practice Exercise 1 For the reaction 4 NH3(g) + 5...Ch. 15.7 - Prob. 15.12.2PECh. 15 - Prob. 1DECh. 15 - Based on the following energy profile, predict...Ch. 15 - 15.2 The following diagrams represent a...Ch. 15 - Prob. 3ECh. 15 - Prob. 4ECh. 15 - Prob. 5ECh. 15 - 15.6 Ethene (C2H4) reacts with healogens (X2) by...Ch. 15 - When lead(IV) oxide is heated above 300 O C, it...Ch. 15 - Prob. 8ECh. 15 - The reactin A2(g) + B(g) + A(g) + AB(g) has an...Ch. 15 - Prob. 10ECh. 15 - Prob. 11ECh. 15 - The following graph represents the yield of the...Ch. 15 - Suppose that the gas-phase reactions A B and B A...Ch. 15 - Prob. 14ECh. 15 - Prob. 15ECh. 15 - Write the expression for KC for the following...Ch. 15 - When the following reaction come to equilibrium,...Ch. 15 - Prob. 18ECh. 15 - Prob. 19ECh. 15 - Prob. 20ECh. 15 - If Kc = 0.042 for PC13(g) + C12 (g) PC15 (g) at...Ch. 15 - Prob. 22ECh. 15 - 15.23 The equilibrium constant for the...Ch. 15 - Prob. 24ECh. 15 - Prob. 25ECh. 15 - Prob. 26ECh. 15 - The following equilibria were attained at 823 K:...Ch. 15 - Consider the equilibrium N2(g) + O2(g) + Br2(g) 2...Ch. 15 - Mercury(I) oxide decomposes into elemental mercury...Ch. 15 - Prob. 30ECh. 15 - Prob. 31ECh. 15 - Prob. 32ECh. 15 - Prob. 33ECh. 15 - Phosphorus trichloride gas and chlorine gas react...Ch. 15 - A mixture of 0.10 mol of NO, 0.050 mol of H2, and...Ch. 15 - Prob. 36ECh. 15 - A mixture of 0.2000 mol of CO2, 0.1000 mol of H2,...Ch. 15 - 15.38 A flask is charged with 1.500 atm of N2O4(g)...Ch. 15 - Prob. 39ECh. 15 - Prob. 40ECh. 15 - a. If QC KC, in which direction will a reaction...Ch. 15 - Prob. 42ECh. 15 - At 100 OC , the equilibrium constant for the...Ch. 15 - 15.44 As shown in Table 15.2, KP for the...Ch. 15 - At 100 C, K = 0.078 for the reaction SO2Cl2 (g) ...Ch. 15 - Prob. 46ECh. 15 - Prob. 47ECh. 15 - Prob. 48ECh. 15 - At 800 k, the equilibrium constant for I2 (g) ...Ch. 15 - Prob. 50ECh. 15 - At 2000 OC, the equilibrium constant for the...Ch. 15 - For the equilibrium Br2 (g) + Cl2 (g) 2BrCl(g) At...Ch. 15 - At 373 k, Kp = 0.416 for the equilibrium 2NOBr (g)...Ch. 15 - At 218 oC, KC= 1.2 X 10-4 for the equilibrium NH4...Ch. 15 - Prob. 55ECh. 15 - At 80 oC, K =1.87 X 10-3 for the reaction PH3 BCl3...Ch. 15 - Prob. 57ECh. 15 - Prob. 58ECh. 15 - Prob. 59ECh. 15 - Prob. 60ECh. 15 - Consider the following equilibrium for which H<0...Ch. 15 - Prob. 62ECh. 15 - 15.63 How do the following changes affect the...Ch. 15 - Prob. 64ECh. 15 - Consider the following equilibrium between oxides...Ch. 15 - Prob. 66ECh. 15 - Ozone, O3, decomposes to molecular oxygen in the...Ch. 15 - Prob. 68ECh. 15 - Prob. 69ECh. 15 - 15.70 True or false: When the temperature of an...Ch. 15 - Prob. 71AECh. 15 - Prob. 72AECh. 15 - 15.73 A mixture of CH4 and H2O is passed over a...Ch. 15 - Prob. 74AECh. 15 - Prob. 75AECh. 15 - Prob. 76AECh. 15 - Prob. 77AECh. 15 - Prob. 78AECh. 15 - Prob. 79AECh. 15 - For the equilibrium PH3BCI3 (s) PH3 (g) + BCI3...Ch. 15 - Prob. 81AECh. 15 - Prob. 82AECh. 15 - Prob. 83AECh. 15 - At 900 o C, Kc = 0.0108 for the reaction CaCO3(g) ...Ch. 15 - Prob. 85AECh. 15 - The equilibrium constant Kc for C(s) +CO2 2CO(g)...Ch. 15 - Prob. 87AECh. 15 - Le Chatelier noted that many industrial processes...Ch. 15 - Prob. 89AECh. 15 - Prob. 90AECh. 15 - [15.91] An equilibrium mixture of H2, I2, and HI...Ch. 15 - Consider the hypothetical reaction A(g) + 2B(g) 2...Ch. 15 - Prob. 93AECh. 15 - Prob. 94AECh. 15 - Prob. 95IECh. 15 - The following equilibria were measured at 823 K:...Ch. 15 - Prob. 97IECh. 15 - Prob. 98IECh. 15 - At 800 K, the equilibrium constant for the...Ch. 15 - Prob. 100IECh. 15 - Prob. 101IECh. 15 - Prob. 102IE
Knowledge Booster
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.Similar questions
- 7-64 As we shall see in Chapter 20, there are two forms of glucose, designated alpha and betawhich are in equilibrium in aqueous solution. The equilibrium constant for the reaction is 1.5 at 30°C. (a) If you begin with a fresh 1.0 M solution of D-glucose in water, what will be its concentration when equilibrium is reached? (b) Calculate the percentage of glucose and of glucose present at equilibrium in aqueous solution at 30°C.arrow_forwardConsider the equation G = G + RT ln(Q). What is the value of G for a reaction at equilibrium? What does Q equal at equilibrium? At equilibrium, the previous equation reduces to G = RT ln(K). When G 0, what does it indicate about K? When G 0, what does it indicate about K? When t G = 0, what does it indicate about K? G predicts spontaneity for a reaction, whereas G predicts the equilibrium position. Explain what this statement means. Under what conditions can you use G to determine the spontaneity of a reaction?arrow_forward7-17 If a certain reaction takes 16 h to go to completion at 10°C, what temperature should we run it if we want it to go to completion in 1 h?arrow_forward
- Consider the following relationships: G = 1, H = TS, Q = 1. G = G, K = 1 Which of these relationships is(are) always true for a reaction at equilibrium?arrow_forwardWhat is the expression for Ke for the following reaction? PC13(g) + Cl2(g) =PC15(g) [PC]3]² / [PC!5] A O [PC|3][Cl2].B O [PC]3][Cl2] / [PC\5] .CO [PC!5] / [PC13][C2] D Oarrow_forward6. Determine the values of Kc that correspond to the following values of Kp a) SO2C12(g) → S02(g) + Cl2(g) Kp = 2.9 x 10-2 at 303K b) 2NO2 (g) + 2NO2(g)+ 02(g) Kp = 0.275 at 700K c) CO(g) + Cl2(g) CoCl,(g) K, = 22.5 at 395°Carrow_forward
- Which of the following statements is FALSE? When K>> 1, the forward reaction is favored and essentially goes to completion. When K= 1, neither the forward or reverse reaction is strongly favored, and about the same amount of reactants and products exist at equilibrium. O When K1 implies that the reaction is very fast at producing products. None of the above.arrow_forwardConsider the following reversible reaction at equilibrium: C6H12O6(aq) + 6 O2(g) 6 CO2(g) + 6 H2O(l). If oxygen gas is removed from the equilibrium reaction vessel, how is the stress relieved?arrow_forward3. The following equilibrium process has been studied at 458°c. NażCO; (s) + S02 (g) +02 (g) )2 NazSO4 (s) + CO2 {g) In one experiment, the amount of the reacting species at equilibrium are found to be [NA2CO3] = 0.645 mole; [SQ2] = 0.65 mole; [O2] = 0.67 mole; [N22SO4] = 1.3 moles; and mole. Assuming that the volume of the gas in the container is 988 ml at 498°C, what is the reaction quotient of the reaction? At what side will the equilibrium shift if the equilibrium constant of the reaction is 1.3 at that temperature? (CO2] = 0.015 %3D %3Darrow_forward
- Nitrogen and hydrogen react to form ammonia, like this: N,(9)+3H,(9)→ 2NH;(g) The reaction is exothermic. Suppose a mixture of N,, H, and NH, has come to equilibrium in a closed reaction vessel. Predict what change, if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. perturbation change in composition shift in equilibrium Oto the right The temperature is lowered. O to the left The pressure of N, will O (none) O to the right O to the left The temperature is raised. The pressure of NH3 will O (none)arrow_forward[obj 13] Plz help with question #5, part B, and show work.arrow_forward105arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Introduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Introduction to General, Organic and Biochemistry
Chemistry
ISBN:9781285869759
Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Chemical Equilibria and Reaction Quotients; Author: Professor Dave Explains;https://www.youtube.com/watch?v=1GiZzCzmO5Q;License: Standard YouTube License, CC-BY