Identify the correct balanced equation and the sign of
Want to see the full answer?
Check out a sample textbook solutionChapter 18 Solutions
Chemistry
- Use S values to calculate the standard entropy change, rS0, for each of the following processes and comment on the sign of the change. (a) KOH(s) KOH(aq) (b) Na(g) Na(s) (c) Br2() Br2(g) (d) HCl(g) HCl(aq)arrow_forwardAt room temperature, the entropy of the halogens increases from I2 to Br2 to Cl2. Explain.arrow_forwardWithout doing any calculations, predict the sign of rS for the following reaction: Zn(s) + 2 HCl(aq) ZnCl2(aq) + H2(g) (a) rS 0 (b) rS = 0 (c) rS 0arrow_forward
- Predict the sign of S, if possible, for each of the following reactions. If you cannot predict the sign for any reaction, state why. a HCl(g)+NH3(g)NH4Cl(s) b N2(g)+3H2(g)2NH3(g) c 2SO2(g)+O2(g)2SO3(g) d CH3OH(l)+32O2(g)CO2(g)+2H2O(g)arrow_forwardImpure nickel, refined by smelting sulfide ores in a blast furnace, can be converted into metal from 99.90% to 99.99% purity by the Mond process. The primary reaction involved in the Mond process is Ni(s)+4CO(g)Ni(CO)4(g) a. Without referring to Appendix 4, predict the sign of S for the above reaction. Explain. b. The spontaneity of the above reaction is temperature-dependent. Predict the sign of Ssurr, for this reaction. Explain c. For Ni(CO)4(g), Hfo=607KJ/mol and S = 417 J/K mol at 298 K. Using these values and data in Appendix 4, calculate H and S for the above reaction. d. Calculate the temperature at which G = 0 (K = 1) for the above reaction, assuming that H and S do not depend on temperature. e. The first step of the Mood process involves equilibrating impure nickel with CO(g) and Ni(CO)4(g) at about 50C. The purpose of this step is to convert as much nickel as possible into the gas phase. Calculate the equilibrium constant for the above reaction at 50.C. f. In the second step of the Mood process, the gaseous Ni(CO)4 is isolated and heated to 227C. The purpose of this step is to deposit as much nickel as possible as pure solid (the reverse of the preceding reaction). Calculate the equilibrium constant for the preceding reaction at 227C. g. Why is temperature increased for the second step of the Mood process? h. The Mond process relies on the volatility of Ni(CO)4 for its success. Only pressures and temperatures at which Ni(CO)4 is a gas are useful. A recently developed variation of the Mood process carries out the first step at higher pressures and a temperature of l52C. Estimate the maximum pressure of Ni(CO)4(g) that can be attained before the gas will liquefy at 152C. The boiling point for Ni(CO)4 is 42C and the enthalpy of vaporization is 29.0 kJ/mol. [Hint: The phase change reaction and the corresponding equilibrium expression are Ni(CO)4(l)Ni(CO)4(g)K=PNi(CO)4 Ni(CO)4(g) will liquefy when the pressure of Ni(CO)4 is greater than the K value.]arrow_forwardConsider two perfectly insulated vessels. Vessel 1 initially contains an ice cube at 0C and water at 0C. Vessel 2 initially contains an ice cube at 0C and a saltwater solution at 0C. Consider the process H2O(s) H2O(l). a. Determine the sign of S, Ssurr, and Suniv for the process in vessel 1. b. Determine the sign of S, Ssurr, and Suniv for the process in vessel 2. (Hint: Think about the effect that a salt has on the freezing point of a solvent.)arrow_forward
- Calculate H and G for the following reactions at 25C, using thermodynamic data from Appendix C; interpret the signs of H and G. a 2PbO(s)+N2(g)2Pb(s)+2NO(g)\ b CS2(l)+2H2O(l)CO2(g)+2H2S(g)arrow_forwardCalculate the entropy change for each of these processes. thereby verifying the predictions made in Conceptual Exercise 16.4. (a) 2 CO2(g) 2 CO(g) + O2(g) (b) NaCl(s) NaCl(aq) (c) MgCO3(s) MgO(s) + CO2(g)arrow_forwardPredict the sign of S and then calculate S for each of the following reactions. a. 2H2S (g) + SO2(g) 3Srhommbic(s) + 2H2O(g) b. 2SO3 (g) 2SO2(g) + O2(g) c. Fe2O3(s) + 3H2(g) 2Fe(s) + 3H2O (g)arrow_forward
- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning