Chemistry: An Atoms First Approach
2nd Edition
ISBN: 9781305079243
Author: Steven S. Zumdahl, Susan A. Zumdahl
Publisher: Cengage Learning
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Chapter 16, Problem 120IP
Interpretation Introduction
Interpretation: The reaction between
Concept introduction: The expression for free energy change is,
The relation between
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What is the free energy change for the following reaction at 25 oC if the entropy change at this temperature is 10 J/K?
3 A (g) + B (s) ------ 2 C (g) + 3.40 kJ
A.) 6380 J B.) – 369 J C.) – 6380 J D.) – 420 J E.) 31020 J
1. What is the free energy change for the following reaction at 25 oC if the entropy change at this temperature is - 10 J/K?3 A (g) + B (s) ------ 2 C (g) + 3.40 kJA. 6380 J B. – 369 J C. – 6380 J D. – 420 J E. 31020 J
Which of the following is TRUE about the Gibbs Free energy?
Select one:
a. It is positive for spontaneous reactions
b. It has the same units as entropy
c. Its absolute value is smallest at equilibrium
d. It the amount of energy needed for a spontaneous reaction to occur
Which of the following hypothetical reactions would most likely be spontaneous only at high temperature?
Select one:
a. 2A(s) + B(aq) --> 2C(g) + D(aq); ΔH > 0
b. 2A(g) + B(g) --> 2C(aq) + D(g); ΔH > 0
c. 2A(g) + B(g) --> 2C(aq) + D(g); ΔH < 0
d. 2A(s) + B(aq) --> 2C(g) + D(aq); ΔH < 0
Chapter 16 Solutions
Chemistry: An Atoms First Approach
Ch. 16 - Define the following: a. spontaneous process b....Ch. 16 - What is the second law of thermodynamics? For any...Ch. 16 - Prob. 3RQCh. 16 - Prob. 4RQCh. 16 - Prob. 5RQCh. 16 - What is the standard free energy change, G, for a...Ch. 16 - If you calculate a value for G for a reaction...Ch. 16 - Consider the equation G = G + RT ln(Q). What is...Ch. 16 - Even if G is negative, the reaction may not occur....Ch. 16 - Prob. 10RQ
Ch. 16 - For the process A(l) A(g), which direction is...Ch. 16 - Prob. 2ALQCh. 16 - Gas A2 reacts with gas B2 to form gas AB at a...Ch. 16 - Prob. 4ALQCh. 16 - Prob. 5ALQCh. 16 - Prob. 6ALQCh. 16 - Predict the sign of S for each of the following...Ch. 16 - Is Ssurr favorable or unfavorable for exothermic...Ch. 16 - At 1 atm, liquid water is heated above 100C. For...Ch. 16 - Prob. 10ALQCh. 16 - The synthesis of glucose directly from CO2 and H2O...Ch. 16 - When the environment is contaminated by a toxic or...Ch. 16 - Entropy has been described as times arrow....Ch. 16 - Prob. 14QCh. 16 - A mixture of hydrogen gas and chlorine gas remains...Ch. 16 - Consider the following potential energy plots: a....Ch. 16 - Prob. 17QCh. 16 - Given the following illustration, what can be said...Ch. 16 - The third law of thermodynamics states that the...Ch. 16 - Prob. 20QCh. 16 - Prob. 21QCh. 16 - Prob. 22QCh. 16 - Monochloroethane (C2H5Cl) can be produced by the...Ch. 16 - Prob. 24QCh. 16 - Which of the following processes are spontaneous?...Ch. 16 - Which of the following processes are spontaneous?...Ch. 16 - Prob. 27ECh. 16 - Consider the following illustration of six...Ch. 16 - Consider the following energy levels, each capable...Ch. 16 - Prob. 30ECh. 16 - Choose the substance with the larger positional...Ch. 16 - Which of the following involve an increase in the...Ch. 16 - Predict the sign of Ssurr for the following...Ch. 16 - Prob. 34ECh. 16 - Given the values of H and S, which of the...Ch. 16 - At what temperatures will the following processes...Ch. 16 - Ethanethiol (C2H5SH; also called ethyl mercaptan)...Ch. 16 - For mercury, the enthalpy of vaporization is 58.51...Ch. 16 - For ammonia (NH3), the enthalpy of fusion is 5.65...Ch. 16 - The enthalpy of vaporization of ethanol is 38.7...Ch. 16 - Predict the sign of S for each of the following...Ch. 16 - Prob. 42ECh. 16 - Prob. 43ECh. 16 - For each of the following pairs, which substance...Ch. 16 - Predict the sign of S and then calculate S for...Ch. 16 - Predict the sign of S and then calculate S for...Ch. 16 - Prob. 47ECh. 16 - Prob. 48ECh. 16 - Prob. 49ECh. 16 - Two crystalline forms of white phosphorus are...Ch. 16 - Consider the reaction 2O(g)O2(g) a. Predict the...Ch. 16 - Prob. 52ECh. 16 - Prob. 53ECh. 16 - The major industrial use of hydrogen is in the...Ch. 16 - Prob. 55ECh. 16 - At 100C and 1.00 atm, H = 40.6 kJ/mol for the...Ch. 16 - Prob. 57ECh. 16 - Prob. 58ECh. 16 - Prob. 59ECh. 16 - Prob. 60ECh. 16 - Consider the reaction...Ch. 16 - Consider the reaction 2POCl3(g)2PCl3(g)+O2(g) a....Ch. 16 - Prob. 63ECh. 16 - Consider two reactions for the production of...Ch. 16 - Prob. 65ECh. 16 - Prob. 66ECh. 16 - Consider the reaction 2NO2(g)N2O4(g) For each of...Ch. 16 - Prob. 68ECh. 16 - One of the reactions that destroys ozone in the...Ch. 16 - Hydrogen sulfide can be removed from natural gas...Ch. 16 - Consider the following reaction at 25.0C:...Ch. 16 - The standard free energies of formation and the...Ch. 16 - Calculate G forH2O(g)+12O2(g)H2O2(g) at 600. K,...Ch. 16 - The Ostwald process for the commercial production...Ch. 16 - Cells use the hydrolysis of adenosine...Ch. 16 - One reaction that occurs in human metabolism is...Ch. 16 - Prob. 77ECh. 16 - Consider the following reaction at 298 K:...Ch. 16 - Prob. 79ECh. 16 - The equilibrium constant K for the reaction...Ch. 16 - Prob. 81AECh. 16 - Some water is placed in a coffee-cup calorimeter....Ch. 16 - Consider the following system at equilibrium at...Ch. 16 - Calculate the entropy change for the vaporization...Ch. 16 - As O2(l) is cooled at 1 atm, it freezes at 54.5 K...Ch. 16 - Prob. 86AECh. 16 - Using the following data, calculate the value of...Ch. 16 - Prob. 88AECh. 16 - Carbon monoxide is toxic because it bonds much...Ch. 16 - Prob. 90AECh. 16 - Prob. 91AECh. 16 - Use the equation in Exercise 79 to determine H and...Ch. 16 - Consider the reaction...Ch. 16 - Consider the following diagram of free energy (G)...Ch. 16 - Prob. 95CWPCh. 16 - For rubidium Hvapo=69.0KJ/mol at 686C, its boiling...Ch. 16 - Given the thermodynamic data below, calculate S...Ch. 16 - Prob. 98CWPCh. 16 - Prob. 99CWPCh. 16 - Consider the dissociation of a weak acid HA (Ka =...Ch. 16 - Prob. 101CWPCh. 16 - The equilibrium constant for a certain reaction...Ch. 16 - For the following reactions at constant pressure,...Ch. 16 - The standard enthalpy of formation of H2O(l) at...Ch. 16 - Prob. 105CPCh. 16 - Liquid water at 25C is introduced into an...Ch. 16 - Using data from Appendix 4, calculate H, G, and K...Ch. 16 - Prob. 108CPCh. 16 - Prob. 109CPCh. 16 - Prob. 110CPCh. 16 - Prob. 111CPCh. 16 - Prob. 112CPCh. 16 - If wet silver carbonate is dried in a stream of...Ch. 16 - Carbon tetrachloride (CCl4) and benzene (C6H6)...Ch. 16 - Sodium chloride is added to water (at 25C) until...Ch. 16 - Prob. 116CPCh. 16 - Prob. 117CPCh. 16 - Prob. 118IPCh. 16 - Prob. 119IPCh. 16 - Prob. 120IPCh. 16 - Consider a sample containing 5.00 moles of a...Ch. 16 - Impure nickel, refined by smelting sulfide ores in...
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- At room temperature, the entropy of the halogens increases from I2 to Br2 to Cl2. Explain.arrow_forwardIndicate which substance in the given pairs has the higher entropy value. Explain your choices.. (a) C2H5OH(l) or C3H7OH(l). (b) C2H5OH(l) or C2H5OH(g). (c) 2H(g) or H(g)arrow_forwardWhich contains greater entropy, a quantity of frozen benzene or the same quantity of liquid benzene at the same temperature? Explain in terms of the dispersal of energy in the substance.arrow_forward
- (11111) Which of the following statements determine a reaction to be spontaneous? The ∆Hrxn is positive. The ∆Suniv is positive. The ∆G0 is positive. The ∆Srxn is positive.arrow_forwardWhich of the following statements concerning entropy is/are CORRECT? 1. The entropy of a substance increases when converted from a liquid to a solid. 2. The entropy of a substance decreases as its temperature increases. 3. All substances have positive standard molar entropies at temperatures above 0 K. a. 1 only b. 2 only c. 3 only d. 1 and 2 e. 1, 2, and 3arrow_forwardWithout consulting the tables, what sign do you expect for the change in entropy (delta S) for the following reaction? 2 C4H10 (g) + 13 O2 (g) → 8 CO2 (g) + 10 H2O (g) a. none of these b. negative c. can not be determined (too close to estimate) d. positivearrow_forward
- predict the sign (+ or -) of the entropy change for the following reaction: I2(l) -> I2(s)arrow_forwardNow calculate the change in entropy (delta S) for the following reaction, using the thermodynamic tables (from your book or on Moodle). 2 C4H10 (g) + 13 O2 (g) → 8 CO2 (g) + 10 H2O (g) Select one: a. – 515 J/K b. 113 J/K c. 515 J/K d. none of these e. – 312 J/K f. 402 J/K g. – 402 J/K h. – 113 J/K i. 312 J/Karrow_forwardConsider the reaction: 2 POCl3 (g) -> 2 PCl3 (g) + O2 (g) A) Calculate DGrxn° for the reaction (DHrxn° = 572 kJ; DSrxn° = 179 J/K) B) Is the reaction spontaneous or not spontaneous? At what temperature would it reach equilibrium?arrow_forward
- 1)non-spontaneous or spontaneous 2)Gibbs free energy is negative or positive 3)positive or negativearrow_forwardWhat is the free energy change for the following reaction at 25 oC if the entropy change at this temperature is - 10 J/molK? 3 A (g) + B (s) ------ 2 C (g) + 3.40 kJ A. - 3.30 kJ/mol B. + 6.38 kJ/mol C. + 0.420 kJ/mol D. - 6.38 kJ/mol E. - 0.420 kJ/molarrow_forwardWhich reaction below is spontaneous at SATP? ∆Hº=14.1 kJ and ∆Sº=49.2 J/K ∆Hº=34.1 kJ and ∆Sº=46.2 J/K ∆Hº=-4.1 kJ and ∆Sº=-52.1 J/K ∆Hº=64.4 kJ and ∆Sº=-2.45 J/Karrow_forward
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