Learning Task 3 Determine if each of the following redox reactions is spontaneous or not. 1. Cu + 2Ag+→ Cu²+ + 2Ag 2. Al³+ + Fe → Al + Fe²+ 3. Zn+ Ni2+ Zn2+ + Ni 4. 3Pb + 2AU3+3Pb2+ + 2AU 5. Hg + Pb2+ Hg2+ + Pb Solve the following problems. 1. A voltaic cell is based on a a Co2+ /Co half-cell and an AgCI/Ag half-cell. a. What reaction occurs at the anode? b. What is the standard cell potential? 2. Using the standard reduction potentials, calculate the standard emf for each of the following reactions: a. 2Al3+ + 3Cd 2A1+3Cd²+ b. Cr+ 2Cr³+→3Cr2+ C. H₂ + 12 → 2H+ + 21- Learning Task 4

Learning Task 3 Determine if each of the following redox reactions is spontaneous or not. 1. Cu + 2Ag+→ Cu²+ + 2Ag 2. Al³+ + Fe → Al + Fe²+ 3. Zn+ Ni2+ Zn2+ + Ni 4. 3Pb + 2AU3+3Pb2+ + 2AU 5. Hg + Pb2+ Hg2+ + Pb Solve the following problems. 1. A voltaic cell is based on a a Co2+ /Co half-cell and an AgCI/Ag half-cell. a. What reaction occurs at the anode? b. What is the standard cell potential? 2. Using the standard reduction potentials, calculate the standard emf for each of the following reactions: a. 2Al3+ + 3Cd 2A1+3Cd²+ b. Cr+ 2Cr³+→3Cr2+ C. H₂ + 12 → 2H+ + 21- Learning Task 4

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter16: Thermodynamics

Section: Chapter Questions

Problem 1E: What is a spontaneous reaction?

See similar textbooks

Similar questions

Consider the reactionNH4Cl(aq)------->NH3(g) + HCl(aq)Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K.ANSWER:
Consider the following reaction at 298K.Cu2+ (aq) + Cr2+ (aq) Cu+ (aq) + Cr3+ (aq)Which of the following statements are correct?Choose all that apply. Eocell > 0 The reaction is reactant-favored. n = 4 mol electrons delta Go > 0 K > 1 Submit Answer
Part A) Consider the reactionI2(g) + Cl2(g)---->2ICl(g)Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K.ANSWER:___________ Part B) Consider the reactionI2(g) + Cl2(g)--->2ICl(g)Use the standard thermodynamic data in the tables linked above. Calculate G for this reaction at 298.15K if the pressure of ICl(g) is reduced to 20.44 mm Hg, while the pressures of I2(g) and Cl2(g) remain at 1 atm.ANSWER: ____________kJ/mol
Part A) Consider the reaction 4 HCl(g) + O2(g)----> 2 H2O(g) + 2 Cl2(g) Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K.ANSWER: __________ Part B) Consider the reactionI2(g) + Cl2(g)---->2ICl(g)Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K.ANSWER:___________ Part C) Consider the reaction2H2O2(l)----->2H2O(l) + O2(g)Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K.ANSWER:__________
Determine which reaction(s) would be spontaneous as written. Select all that apply Cu2+(aq)+2Fe2+ (aq)--> Cu(s)+2Fe3+(aq) 3Cu2+(aq)+2Fe (s)--> 3Cu(s)+2Fe3+(aq) 2Fe3+(aq)+Cu (s)--> 2Fe2+(aq)+Cu2+(aq) 2Fe3+(aq)+3Cu (s)--> 2Fe(s)+3Cu2+(aq)
Consider the reactionCa(OH)2(aq) + 2 HCl(aq) ----> CaCl2(s) + 2 H2O(l)Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K.ANSWER: ____________
Determine which reaction(s) would be spontaneous as written. Select all that apply Cu2+(aq)+2Fe2+ (aq)--> Cu(s)+2Fe3+(aq) 3Cu2+(aq)+2Fe (s)--> 3Cu(s)+2Fe3+(aq) 2Fe3+(aq)+Cu (s)--> 2Fe2+(aq)+Cu2+(aq) 2Fe3+(aq)+3Cu (s)--> 2Fe(s)+3Cu2+(aq) the answer is (but I'm not sure how it's this): 3Cu2+(aq)+2Fe (s)--> 3Cu(s)+2Fe3+(aq) 2Fe3+(aq)+Cu (s)--> 2Fe2+(aq)+Cu2+(aq)
Consider the reactionI2(g) + Cl2(g)2ICl(g)Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K.ANSWER:
Please do this correctly neat and clean...(posting it second time) Consider the corrosion of copper at 30°C using the overall reaction: Cu(s) + 0.5 O2(g) + 2 H3O+(aq) → Cu2+(aq) + 3 H2O(l) If the partial pressure of oxygen is 0.88 bar, and the concentration of Cu2+(aq) is 5.1 M, at what pH does the reaction become spontaneous?
Will the following reaction occur spontaneously at 250C if [Fe2+] = 0.060 M and [Cd2+] = 0.60 M? Fe2+(aq) + Cd(s) -----> Fe(s) + Cd2+(aq)? (Use Nernst equation to solve this problem and Eo Cd2+ = -0.40 and Fe2+ = -0.44).
A reaction with a positive ΔG cannot proceed in any circumstances. Select one: True False
PCl3 + 3 CH3CH2OH --> 3 CH3CH2Cl + H3PO3 Compound ΔGof, kJ/mol Sfo, J/mol-K PCl3 -286 312 CH3CH2OH -175 161 CH3CH2Cl -53 190 H3PO3 -232 82 A. Find ΔGorxn. B. Is the reaction spontaneous at 25oC? C. Find ΔSorxn. D. Find ΔHorxn.