Practice ProblemBUILD
Want to see the full answer?
Check out a sample textbook solutionChapter 18 Solutions
CHEMISTRY LOOSELEAF TEXT W/CONNECT >IP
- Predict the sign of ΔS°, if possible, for the following reaction. A. N2(g) + O2(g) ----> 2NO(g) B. C2H2(g) + 2H2(g) ----> C2H6(g) Question 3 options: positive negative not predictablearrow_forwardFor the reaction CaCO3(s) → CaO(s) + CO2(g) which is spontaneous only at high temperatures Group of answer choices ∆H is positive and ∆S is positive ∆H is negative and ∆S is positive ∆H is positive and ∆S is negative ∆H is negative and ∆S is negativearrow_forwardFor which of the following is the change in entropy positive? Check all that apply. Explain. A. C 6 H 12 (l) C 6 H 12 (g)B. Dilution of 1.0 mL of 1.0 M NaOH with 90 mL of waterC. . 2 O 2 (g) + 2 SO (g) 2 SO 3 (g)D. grinding a large crystal of NaCl to powderE. Cooling water from room temperature to 15°C.arrow_forward
- Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction. CaCO3(s) → CaO(s) + CO2(g) ΔG° =+131.1 kJ P(CO2) = 0.033 atm A) -49.3 kJ B) -8.32 kJ C) +122.6 kJ D) +39.7 kJ E) +43.3 kJarrow_forwardConsider the reaction Fe(s) + 2 HCl(aq) → FeCl2(s) + H2(g) Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K. ANSWER: _______arrow_forwardWhat is the sign of ΔS for the reaction Na2B4O7(s) 2 Na+(aq) + B4O72-(aq) ?arrow_forward
- The combination of ΔH and ΔS for a process that will always be nonspontaneous is _____. ΔH is positive and ΔS is positive ΔH is negative and ΔS is positive ΔH is negative and ΔS is negative ΔH is positive and ΔS is negativearrow_forwardUsing ΔG = ΔH – TΔS, explain under what circumstances the following processes would be spontaneous: a. ΔH<0 and ΔS>0 b. ΔH>0 and ΔS<0 c. ΔH<0 and ΔS<0 d. ΔH>0 and ΔS>0arrow_forwardH3. Consider a reaction for which the value of ΔG∘ = -9.199 kJ/mol at a 298.15 K. What is the value of Keq for this reaction at this temperature? Please give typed answerarrow_forward
- At 298 K, ΔH° for this reaction is -137.5 kJ/mol, and ΔS° is +120.5 J/K. What is the value of ΔG° (in kJ/mol) at 25 °C for the following the reaction? C₂H₄ (g) + H₂ (g) → C₂H₆ (g)arrow_forwardSelect the circumstances under which a reaction would most likely be spontaneous. a. delta H is positive, delta S is positive, and the temperature is low. b. delta H is positive, delta S is negative, and the temperature is low. c. delta H is positive, delta S is negative, and the temperature is high. d. delta H is negative, delta S is negative, and the temperature is high. e. delta H is negative, delta S is positive, and the temperature is high.arrow_forwardCalculate ΔGrxn at 308 K under the conditions shown below for the following reaction. Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g) ΔG° = -28.0 kJ P(CO) = 1.4 atm, P(CO2) = 2.1 atm Group of answer choices +30.0 kJ +31.1 kJ +24.9 kJ -24.9 kJ -31.1 kJarrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
- Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning