Chemical Principles
8th Edition
ISBN: 9781305581982
Author: Steven S. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Chapter 10, Problem 73E
Hydrogen sulfide can be removed from natural gas bythe reaction
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Chapter 10 Solutions
Chemical Principles
Ch. 10 - For the process A(l)A(g) , which direction is...Ch. 10 - Prob. 2DQCh. 10 - Prob. 3DQCh. 10 - Prob. 4DQCh. 10 - Prob. 5DQCh. 10 - Prob. 6DQCh. 10 - Predict the sign of S for each of the following...Ch. 10 - Prob. 8DQCh. 10 - Prob. 9DQCh. 10 - At 1 atm, liquid water is heated above 100°C. For...
Ch. 10 - Prob. 11DQCh. 10 - Prob. 12ECh. 10 - Prob. 13ECh. 10 - Prob. 14ECh. 10 - Consider the following energy levels, each capable...Ch. 10 - Prob. 16ECh. 10 - Prob. 17ECh. 10 - Which of the following involve an increase in the...Ch. 10 - Prob. 19ECh. 10 - Choose the substance with the larger positional...Ch. 10 - In the roll of two dice, what total number is the...Ch. 10 - Entropy can be calculated by a relationship...Ch. 10 - Calculate the energy required to change the...Ch. 10 - For nitrogen gas the values of CvandCp at 25°Care...Ch. 10 - Consider a rigid, insulated box containing 0.400...Ch. 10 - One mole of an ideal gas is contained in a...Ch. 10 - One mole of an ideal gas with a volume of 1.0 L...Ch. 10 - A cylinder with an initial volume of 10.0 L is...Ch. 10 - The molar heat capacities for carbon dioxide at...Ch. 10 - The molar entropy of helium gas at 25°C and 1.00...Ch. 10 - Consider the process A(l)A(g)75C155C which is...Ch. 10 - A sample of ice weighing 18.02 g, initially at...Ch. 10 - Calculate the entropy change for a process in...Ch. 10 - Calculate the change in entropy that occurs...Ch. 10 - The synthesis of glucose directly from CO2andH2O...Ch. 10 - A green plant synthesizes glucose by...Ch. 10 - Entropy has been described as “time’s arrow.”...Ch. 10 - For a gas phase reaction, what do you concentrate...Ch. 10 - What determines Ssurr for a process? To calculate...Ch. 10 - Predict the sign of Ssurr for the following...Ch. 10 - Calculate Ssurr for the following reactions at...Ch. 10 - For each of the following pairs of substances,...Ch. 10 - Predict the sign of S for each of the following...Ch. 10 - Prob. 44ECh. 10 - Prob. 45ECh. 10 - For the reaction CS2(g)+3O2(g)CO2(g)+2SO2(g) S is...Ch. 10 - For the reaction C2H2(g)+4F2(g)2CF4(g)+H2(g) S is...Ch. 10 - Ethanethiol ( C2H5SH ; also called ethyl...Ch. 10 - For mercury at 1 atm, the enthalpy of vaporization...Ch. 10 - The enthalpy of vaporization of ethanol is 38.7...Ch. 10 - For ammonia (NH3) the enthalpy of fusion is 5.65...Ch. 10 - It is quite common for a solid to change from one...Ch. 10 - As O2(l) is cooled at 1 atm, it freezes at 54.5 K...Ch. 10 - Prob. 54ECh. 10 - The value of G for the reaction...Ch. 10 - Of the functions H,S,andG , which dependsmost...Ch. 10 - For the reaction at 29° K, 2NO2(g)N2O4(g) the...Ch. 10 - Consider the reaction...Ch. 10 - Consider the reaction 2POCl3(g)2PCl3(g)+O2(g) a....Ch. 10 - Consider two reactions for the production of...Ch. 10 - Prob. 61ECh. 10 - Prob. 62ECh. 10 - When most biological enzymes are heated, they...Ch. 10 - For the reaction 2O(g)O2(g) a. predict the signs...Ch. 10 - Hydrogen cyanide is produced industrially by the...Ch. 10 - A reaction at constant T and P is spontaneous as...Ch. 10 - G predicts spontaneity for a reaction at constant...Ch. 10 - Using thermodynamic data from Appendix 4,...Ch. 10 - Prob. 69ECh. 10 - Using data from Appendix 4, calculate G for...Ch. 10 - Prob. 71ECh. 10 - One of the reactions that destroys ozone in the...Ch. 10 - Hydrogen sulfide can be removed from natural gas...Ch. 10 - Consider the autoionization of water at 25°C:...Ch. 10 - How can one estimate the value of K at...Ch. 10 - The standard free energies of formation and the...Ch. 10 - Consider the reaction...Ch. 10 - Prob. 78ECh. 10 - Consider the following reaction at 800. K:...Ch. 10 - Consider the following reaction at 298 K:...Ch. 10 - For the reaction A(g)+2B(g)C(g) the initial...Ch. 10 - Consider the following diagram of free energy (G)...Ch. 10 - Calculate G for H2O(g)+12O2(g)H2O2(g) at600. K,...Ch. 10 - Cells use the hydrolysis of adenosine...Ch. 10 - Carbon monoxide is toxic because it bonds much...Ch. 10 - One reaction that occurs in human metabolism is...Ch. 10 - At 25.0°C, for the reaction 2NO2(g)N2O4(g) the...Ch. 10 - Consider the relationship ln(K)=HRT+SR The...Ch. 10 - a. Use the equation in Exercise 88 to determine H...Ch. 10 - The equilibrium constant K for the reaction...Ch. 10 - The equilibrium constant for a certain reaction...Ch. 10 - A sample of a monatomic ideal gas at 1.00 atm...Ch. 10 - A sample of 1.75 moles of H2(Cv=20.5JK-1mol-1) at...Ch. 10 - A 1.50-mole sample of an ideal gas is allowed to...Ch. 10 - Consider 1.00 mole of CO2(g) at 300. K and 5.00...Ch. 10 - Prob. 96ECh. 10 - A mixture of hydrogen gas and chlorine gas...Ch. 10 - When the environment is contaminated by a toxic...Ch. 10 - If you calculate a value for G for a reaction...Ch. 10 - Given the following illustration, what can be said...Ch. 10 - Some water is placed in a coffee cup calorimeter....Ch. 10 - Using Appendix 4 and the following data, determine...Ch. 10 - Prob. 103AECh. 10 - Human DNA contains almost twice as much...Ch. 10 - The enthalpy of vaporization of chloroform (CHCl3)...Ch. 10 - Two crystalline forms of white phosphorus are...Ch. 10 - Monochloroethane (C2H5Cl) can be produced by...Ch. 10 - Acrylonitrile is the starting material used in the...Ch. 10 - Prob. 109AECh. 10 - Many biochemical reactions that occur in cells...Ch. 10 - Consider the following reaction at 35°C:...Ch. 10 - Consider the reaction H2(g)+Br2(g)2HBr(g) where...Ch. 10 - At 1500 K the process I2(g)2I(g)10atm10atm is not...Ch. 10 - Using the following data, calculate the value of...Ch. 10 - Sodium chloride is added to water (at 25°C) until...Ch. 10 - Prob. 116AECh. 10 - Prob. 117AECh. 10 - The deciding factor on why HF is a weak acid and...Ch. 10 - Prob. 119AECh. 10 - Calculate the entropy change for the vaporization...Ch. 10 - The standard entropy values (S°) for...Ch. 10 - Calculate the values of S and G for each of the...Ch. 10 - Calculate the changes in free energy, enthalpy,...Ch. 10 - Consider the isothermal expansion of 1.00 mole of...Ch. 10 - A 1.00-mole sample of an ideal gas in a vessel...Ch. 10 - One mole of an ideal gas with a volume of 6.67 L...Ch. 10 - Which of the following reactions (or processes)...Ch. 10 - For rubidium Hvap=69.0kJ/mol at 686°C, its...Ch. 10 - Given the thermodynamic data below, calculate S...Ch. 10 - Consider the reaction: H2S(g)+SO2(g)3S(g)+2H2O(l)...Ch. 10 - The following reaction occurs in pure water:...Ch. 10 - Consider the dissociation of a weak acid HA...Ch. 10 - Consider the reaction: PCl3(g)+Cl2(g)PCl5(g) a....Ch. 10 - The equilibrium constant for a certain reaction...Ch. 10 - Consider a 2.00-mole sample of Ar at 2.00 atm...Ch. 10 - Prob. 136CPCh. 10 - One mole of an ideal gas undergoes an isothermal...Ch. 10 - At least some of what is in the following quoted...Ch. 10 - You have a 1.00-L sample of hot water (90.°C)...Ch. 10 - Consider two perfectly insulated vessels. Vessel 1...Ch. 10 - If wet silver carbonate is dried in a stream of...Ch. 10 - Consider a weak acid HX. If a 0.10 M solution of...Ch. 10 - Using data from Appendix 4, calculate H , G , and...Ch. 10 - One mole of a monatomic ideal gas (for which...Ch. 10 - Consider the system A(g)B(g) a. 25°C. a. Assuming...Ch. 10 - Liquid water at 25°C is introduced into an...Ch. 10 - Consider 1.00 mole of an ideal gas that is...Ch. 10 - Prob. 148CPCh. 10 - Consider the reaction 2CO(g)+O2(g)2CO2(g) a. Using...Ch. 10 - Prob. 150CPCh. 10 - Prob. 151CPCh. 10 - Consider the following Cp values for N2(g) :...Ch. 10 - Benzene (C6H6) has a melting point of 5.5°C and...Ch. 10 - Prob. 154MPCh. 10 - Prob. 155MP
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- Use the data in Appendix J to calculate rG andKPat 25 C for the reaction 2HBr(g)+Cl2(g)2HCl(g)+Br2() Comment on the connection between the sign of rG and the magnitude ofKP.arrow_forwardA crucial reaction for the production of synthetic fuels is the production of H2 by the reaction of coal with steam. The chemical reaction is C(s) + H2O(g) CO(g) + H2(g) (a) Calculate rG for this reaction at 25 C, assuming C(s) is graphite. (b) Calculate Kp for the reaction at 25 C. (c) Is the reaction predicted to be product-favored at equilibrium at 25 C? If not, at what temperature will it become so?arrow_forwardWhat is the sign of the standard Gibbs free-energy change at low temperatures and at high temperatures for the explosive decomposition of TNT? Use your knowledge of TNT and the chemical equation, particularly the phases, to answer this question. (Thermodynamic data for TNT are not in Appendix G.) 2C7H5N3O6(s) 3N2(g) + 5H2O() + 7C(s) + 7CO(g)arrow_forward
- Calculate the standard Gibbs free-energy change when SO3 forms from SO2 and O2 at 298 K. Why is sulfur trioxide an important substance to study? (Hint: What happens when it combines with water?)arrow_forwarda Calculate K1, at 25C for sulfurous acid: H2SO3(aq)H+(aq)+HSO3(aq) b Which thermodynamic factor is the most significant in accounting for the fact that sulfurous acid is a weak acid? Why?arrow_forwardElemental boron, in the form of thin fibers, can be made by reducing a boron halide with H2. BCl3(g) + 3/2 H2(g) B(s) + 3HCl(g) Calculate H, S, and G at 25 C for this reaction. Is the reaction predicted to be product favored at equilibrium at 25 C? If so, is it enthalpy driven or entropy driven?arrow_forward
- Silver carbonate, Ag2CO3, is a light yellow compound that decomposes when heated to give silver oxide and carbon dioxide: Ag2CO3(s)Ag2O(s)+CO2(g) A researcher measured the partial pressure of carbon dioxide over a sample of silver carbonate at 220C and found that it was 1.37 atm. Calculate the partial pressure of carbon dioxide at 25C. The standard enthalpies of formation of silver carbonate and silver oxide at 25C are 505.9 kJ/mol and 31.05 kJ/mol, respectively. Make any reasonable assumptions in your calculations. State the assumptions that you make, and note why you think they are reasonable.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_forwardAdenosine triphosphate, ATP, is used as a free-energy source by biological cells. (See the essay on page 624.) ATP hydrolyzes in the presence of enzymes to give ADP: ATP(aq)+H2O(l)ADP(aq)+H2PO4(aq);G=30.5kJ/molat25C Consider a hypothetical biochemical reaction of molecule A to give molecule B: A(aq)B(aq);G=+15.0kJ/molat25C Calculate the ratio [B]/[A] at 25C at equilibrium. Now consider this reaction coupled to the reaction for the hydrolysis of ATP: A(aq)+ATP(aq)+H2O(l)B(aq)+ADP(aq)+H2PO4(aq) If a cell maintains a high ratio of ATP to ADP and H2PO4 by continuously making ATP, the conversion of A to B can be made highly spontaneous. A characteristic value of this ratio is [ATP][ADP][H2PO4]=500 Calculate the ratio [B][A] in this case and compare it with the uncoupled reaction. Compared with the uncoupled reaction, how much larger is this ratio when coupled to the hydrolysis of ATP?arrow_forward
- For the decomposition of formic acid, HCOOH(l)H2O(l)+CO(g) H = +29 kJ/mol at 25C. a Does the tendency of this reaction to proceed to a state of minimum energy favor the formation of water and carbon monoxide or formic acid? Explain. b Does the tendency of this reaction to proceed to a state of maximum entropy favor the formation of products or reactants? Explainarrow_forwardThe decomposition of diamond to graphite [C(diamond) C(graphite)] is thermodynamically favored, but occurs slowly at room temperature. a. Use fG values from Appendix L to calculate rG and Keq for the reaction under standard conditions and 298.15 K. b. Use fH and S values from Appendix L to estimate rG and Keq for the reaction at 1000 K. Assume that enthalpy and entropy values are valid at these temperatures. Does heating shift the equilibrium toward the formation of diamond or graphite? c. Why is the formation of diamond favored at high pressures? d. The phase diagram shows that diamond is thermodynamically favored over graphite at 20,000 atmospheres pressure (about 2 GPa) at room temperature. Why is this conversion actually done at much higher temperatures and pressures?arrow_forwardElemental boron, in the form of thin fibers, can be made by reducing a boron halide with H2. BCl3(g) + 32 H2(g) B(s) + 3 HCl(g) Calculate rH, rS, and rG at 25 C for this reaction. Is the reaction predicted to be product-favored at equilibrium at 25 C? If so, is it enthalpy- or entropy-driven? [S for B(s) is 5.86 J/K mol.]arrow_forward
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