Tables_for_Oxidation_Reduction

Tables for Oxidation Reduction 1. Consider the following reactions. Ce 3+ (aq) + 3e -  Ce(s) E o = -2.34 V Cr 2+ (aq) + 2e -  Cr(s) E o = -0.91 V When a spontaneous electrochemical cell is constructed on the basis of the following two half- reactions, the oxidizing agents will gain ______. a six less electrons than the reducing agent gains b two more electrons than the reducing agent loses c three more electrons than the reducing agent loses d the same number of electrons as the reducing agent loses 2. Consider the following reactions. Cl 2 (g) + 2e -  2Cl - (aq) E o = 1.36 V Fe 3+ (aq) + e -  Fe 2+ (aq) E o = 0.77 V Cr 2+ (aq)  Cr 3+ (aq) + e - E o = 0.41V Zn 2+ (aq) + 2e -  Zn(s) Eo = -0.76 V Which chemical species loses electrons? a Cl 2 (g) b Fe 3+ (aq) c Cr 2+ (aq) d Zn 2+ (aq) 3. Which half-reaction has a negative E o value? a Fe 2+ (aq)  Fe 3+ (aq) + e - b Br 2 (l) + 2e -  2Br - (aq) c Au 3+ (aq) + 3e -  Au(s) d Cr(s)  Cr 2+ (aq) + 2e - 4. Which of these would react spontaneously with Co(s) but NOT with H 2 (g)? a H 2 O(l) b Ni 2+ (aq) c Ca 2+ (aq) d Br - (aq)

5. Brad and Charles observed the reactions between four different metals and the solutions of their metallic ions. The boys recorded these "spontaneous" reactions. Reaction I W(s) + X + (aq)  W + (aq) + X(s) II X(s) + Y + (aq)  X + (aq) + Y(s) III Y(s) + Z + (aq)  Y + (aq) + Z(s) IV Z(s) + W + (aq)  Z + (aq) + W(s) V X(s) + Z + (aq)  X + (aq) + Z(s) If equation I is correct, which equation did the student record incorrectly ? a II b III c IV d V 6. Consider the following reactions. 2A + (aq) + Mg(s)  Mg 2+ (aq) + 2A(s) E o = 2.60 V B(s) + Cd 2+ (aq)  Cd(s) + B 2+ (aq) E o = 0.63 V The E o for the reaction 2A + (aq) + B(s)  B 2+ (aq) + 2A(s) is _______ V a 3.23 b 1.97 c 1.26 d 0.80 7. Consider the following reactions Ir(s) +3 Tl + (aq)  Ir 3+ (aq) + 3Tl(s) Negative E o Ir 3+ (aq) + Rh(s)  Ir(s) + Rh 3+ (aq) Negative E o 3Tl + (aq) + Y(s)  3Tl(s) + Y 3+ (aq) Positive E o In these reactions, the strongest oxidizing agent is ____________ a Tl - (aq) b Y 3+ (aq) c Ir 3+ (aq) d Rh 3+ (aq)

13. Consider the oxidation potential table given below. C(s)  C 3+ (aq) + 3e - E o = +1.80 V D(l)  D 2+ (aq) + 2e - E o = +0.35 V A 2+ (aq)  A 4+ (aq) + 2e - E o =-0.25 V 2B - (aq)  B 2 (g) + 2e - E o = -1.25 V The strongest oxidizing agent in this table is _________________ a C(s) b B 2 (g) c A 4+ (aq) d D 2+ (aq) 14. Zinc metal will not spontaneously act as a reducing agent for which group of chemical agents? a Fe 2+ (aq) , H + (aq), Cu 2+ (aq) b Co 2+ (aq), Sn 2+ (aq), Pb 2+ (aq) c Cu 2+ (aq), Hg 2+ (aq), Br 2 (l) d Ca 2+ (aq), Na + (aq), Mn 2+ (aq) 15. The standard electrode potential for the conversion of Sn 2+ (aq) to Sn 4+ (aq) is ___ V a +0.15 b -0.14 c -0.15 d +0.14 16. Consider the following spontaneous reactions, X 2+ (aq) +Y(s)  Y 2+ (aq) + X(s) X 2+ (aq) + Q(s)  X(s) + Q 2+ (aq) Y 2+ (aq) + Z(s)  Y(s) + Z 2+ (aq) Z 2+ (aq) + Q(s)  Z(s) + Q 2+ (aq) Based on this information, the strongest oxidizing agent is ___________ a Q 2+ (aq) b X 2+ (aq) c Z 2+ (aq) d Y 2+ (aq)

17. Consider the following spontaneous reactions, X 2+ (aq) +Y(s)  Y 2+ (aq) + X(s) X 2+ (aq) + Q(s)  X(s) + Q 2+ (aq) Y 2+ (aq) + Z(s)  Y(s) + Z 2+ (aq) Z 2+ (aq) + Q(s)  Z(s) + Q 2+ (aq) Based on this information, the strongest reducing agent is ___________ a Q(s) b X (s) c Z(s) d Y(s) 18. Given the reaction 2NO 3 - (aq) + 4H + (aq) + X(s)  2H 2 O(l) + N 2 O 4 (g) + X 2+ (aq) E o = +2.18 V The standard electrode potential for the half-reaction X 2+ (aq) + 2e -  X(s) is ___ V a +2.98 b +1.38 c -1.38 d -2.98 19. Given the reaction 2NO 3 - (aq) + 4H + (aq) + X(s)  2H 2 O(l) + N 2 O 4 (g) + X 2+ (aq) E o = +2.18 V The standard electrode potential for the half-reaction X(s)  X 2+ (aq) + 2e - is ___ V a +2.98 b +1.38 c -1.38 d -2.98 20. Which process listed below could NOT cause M 3+ (aq) to change to M 2 (g) a R(s)  R 2- (aq) b D 2- (aq)  D + (aq) c T - (aq)  T(s) d L 3- (aq)  L - (aq)

a L + X 2+ R 3+ J b J - R 2+ X L c L X R 2+ J - d J R 3+ X 2+ L + 25. Sue and Amy use the following data to build a reduction table. Each reaction is listed as spontaneous or non spontaneous. R 3+ J X 2+ L + R 2+ Non spontaneous Spontaneous Non spontaneous Non spontaneous J - Non spontaneous Non spontaneous Non spontaneous Non spontaneous X Spontaneous Spontaneous Non spontaneous Non spontaneous L Spontaneous Spontaneous Spontaneous Non spontaneous The reducing agents , listed from the strongest to the weakest will be ___, ____, ____, and ____. a L + X 2+ R 3+ J b J - R 2+ X L c L X R 2+ J - d J R 3+ X 2+ L + 26. Numerical response question Left justify your answer in the boxes provided. 27. Students make the following observations for a series of electrochemical cells 5 6 7 8 Be 2+ Cd 2+ Ra 2+ V 2+ 1 Be (s) x  x  2 Cd (s) x x x x 3 Ra (s)   x  4 V (s) x  x x  Indicates a spontaneous reaction X Indicates a non-spontaneous reaction

Using the assigned numbers from 1 to 8, list the oxidizing agents in order from strongest to weakest. ___, ___, ___, ___ 28. Numerical response question Left justify your answer in the boxes provided. Students make the following observations for a series of electrochemical cells 1 2 3 4 A + (aq) B + (aq) C + (aq) D + (aq) 5 A (s) x  x  6 B (s) x x x x 7 C (s)   x  8 D (s) x  x x  Indicates a spontaneous reaction X Indicates a non-spontaneous reaction Using the assigned numbers from 1 to 8, list the reducing agents in order from strongest to weakest. ___, ___, ___, ___ 29. Numerical response question Left justify your answer in the boxes provided. Students make the following observations for a series of electrochemical cells 1 2 3 4 A + (aq) B + (aq) C + (aq) D + (aq) 5 A (s) x x x  6 B (s)  x  

Solutions: 1. D 2. C 3. A 4. B 5. C 6. C 7. D 8. C 9. A 10. D 11. A 12. C 13. B 14. D 15. C 16. B 17. A 18. C 19. b 20. A 21. A 22. B 23. C 24. D 25. C 26. 6857 27. 7586 28. 6758 29. 4123 30. 1126 31. 3.16