From each of the following pairs of substances, use data in Appendix E in the textbook to choose the one that is the stronger oxidizing agent.
Match the words in the left column to the appropriate blanks in the sentences on the right. Make certain each sentence is complete before submitting your answer.
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Higher the value of standard reduction potential of a compound, it will have strong tendency to get reduced and oxidize the other compound. The compound with higher reduction potential will be stronger oxidizing agent.
Zn2+(aq) + 2e-Zn(s). E° = -0.76V
Fe2+(aq) +2e-Fe(s) . E° = -0.44V
(1) the stronger oxidizing agent is Fe2+(aq). (Answer)
H2O2 +2H+ + 2e- O2 + 2H2O . E° = 1.78V
O3 + 2H+ + 2e- O2 + H2O. E° = 2.07V
(2)the stronger oxidizing agent is O3(g). (Answer)
Cl2(g) + 2e-2Cl-(aq). E° = 1.36V
2HClO(aq) + 2H+ + 2e- Cl2 + 2H2O. E° = 1.63V
(3) the stronger oxidizing agent is HClO(aq) . (Answer)
F2(g) + 2e-2F-(aq). E° = 2.87V
I2(s) + 2e- 2I-(aq). E° = 0.54V
(4) the stronger oxidising agent is F2(g) . (Answer)
From each of the following pairs of substances, use data in Appendix E in the textbook...
From each of the following pairs of substances, use data in Appendix E in the textbook to choose the one that is the stronger oxidizing agent. Match the words in the left column to the appropriate blanks in the sentences on the right. Make certain each sentence is complete before submitting your answer. ResetHelp HClO(aq) O3(g) H2O2(aq) Zn2+(aq) Fe2+(aq) Cl2(g) F2(g) I2(s) Given Zn2+(aq) or Fe2+(aq) , the stronger oxidizing agent is .GivenH2O2(aq)orO3(g), the stronger oxidizing agent is blank. .GivenCl2(g)orHClO(aq),...
Questions I. Based on the Reduction Potential Table constructed in this experiment: For each of the following, circle the stronger oxidizing agent: i. Ht or Fe3* ii. Cl2 or Zn2 iii. 2 or Br2 a. b. For each of the following, circle the weaker reducing agent: i. Cu or H2 ii. Br or I iii. H2 or Br Predict if he following redox rescióons will be pontaneous (S), r non- spontaneous (N): i. 2H+(aq) + 21-(aq)-- H2(g) + 12(aq) ii....
a. Cl2 b. F2 c. Br2 d. I2 e. All of the halogens have equal strength as oxidizing agents. E°(V +2.87 +1.359 +1.065 +1.23 +0.799 Table 20.1 Half Reaction F2 (8) 2e → 2F- (ag) Cl2(8) 2e → 2Cl- (aq) Br21) 2e → 2Br" (ag) 02 (elut 4H+ (ag) + 4e + 2H20 (1) Agte → Ag (5) Fe3+ (aq) → Fe2+ (aq) 12 (5) + 2e – 21 (ag) Cu2+ + 2e - Cu (s) 2H+ + 2e →...
Part 1.) Using data found in Appendix E of your textbook calculate the nonstandard emf for each of the following reactions if the concentration of each of the ions in these reactions is 0.0002 molar and everything else is standard (use 298 K for the temperature, R = 8.314 J/mol-K, and F = 96,485 C/mol): (a) 2 Hg2+(aq) + 1 Sn(s) --> 1 Hg22+(aq) + 1 Sn2+(aq) E = __ V (b) 1 F2(g) + 1 Mg(s) --> 2 F-(aq)...
Using data found in Appendix E of your textbook calculate the nonstandard emf for each of the following reactions if the concentration of each of the ions in these reactions is 0.0007 molar and everything else is standard (use 298 K for the temperature, R = 8.314 J/mol-K, and F = 96,485 C/mol): (a) 2 Li+(aq) + 1 Sn(s) --> 2 Li(s) + 1 Sn2+(aq) (b) 1 Zn2+(aq) + 1 Ca(s) --> 1 Zn(s) + 1 Ca2+(aq) (c) 1 Mg2+(aq)...
Using data found in Appendix E of your textbook calculate the nonstandard emf for each of the following reactions if the concentration of each of the ions in these reactions is 0.0006 molar and everything else is standard (use 298 K for the temperature, R = 8.314 J/mol-K, and F = 96,485 C/mol): (a) 2 H+(aq) + 2 Cu(s) --> 1 H2(g) + 2 Cu+(aq) E = V (b) 1 Ca2+(aq) + 2 K(s) --> 1 Ca(s) + 2 K+(aq) E...
For each of the following pairs of substances, determine which has the larger molar entropy at 298 K: (A) Br2(l) or (B) Cl2(g) (C) Fe(s) or (D) Ni(s) (E) C2H6(g) or (F) C2H4(g) (G) CH4(g) or (H) CCl4(g) (I) MgO(s) or (J) HgO(s) (K) NaCl(aq) or (L) MgCl2(aq) Enter the six letters in order (e.g. ACEGIK, BDFHJL, etc.)
Use data from Appendix IIB in the textbook to calculate ΔrS∘ for each of the following reactions. CO(g)+2H2(g)→CH3OH(g) Express your answer using four significant figures. ΔrS∘ = JK−1mol−1
Using data found in Appendix E of your textbook calculate the nonstandard emf for each of the following reactions if the concentration of each of the ions in these reactions is 0.0005 molar and everything else is standard (use 298 K for the temperature, R = 8.314 J/mol-K, and F = 96,485 C/mol): Using data found in Appendix E of your textbook calculate the nonstandard emf for each of the following reactions if the concentration of each of the ions...
Use data from Appendix IIB in the textbook to calculate ΔS∘rxn for each of the following reactions. C2H4(g)+H2(g)→C2H6(g) MgCO3(s)→MgO(s)+CO2(g) CO(g)+H2O(g)→H2(g)+CO2(g) 2H2S(g)+3O2(g)→2H2O(l)+2SO2(g)