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Answer: C.Cytochrome a-Fe+2 (-0.29V)
The agent with the highest negative redox potential will be a strong reducing agent, while the one with the highest positive redox potential will be a strong oxidizing agent.
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Question 10 of 43 2O Points Which of the following is...
Consider the following half-reactions: Half-reaction E° (V) 12(s) + 2e - →21"(aq) 0.535V 2H+ (aq) +...
Consider the following half-reactions: Half-reaction E° (V) 12(s) + 2e - →21"(aq) 0.535V 2H+ (aq) + 2e - → H2(g) 0.000V Cr3+(aq) + 3e —— Cr(s) -0.740V The strongest oxidizing agent is: enter formula The weakest oxidizing agent is: The weakest reducing agent is: The strongest reducing agent is: Will 12(s) reduce Cr3+(aq) to Cr(s)? — Which species can be reduced by H2(g)? If none, leave box blank. Use the References to access important values if needed for this question....
help with these please Consider the following half-reactions: Half-reaction Eo (V) F2(g)+ 2e 2F (aq) 2.870V...
help with these please
Consider the following half-reactions: Half-reaction Eo (V) F2(g)+ 2e 2F (aq) 2.870V Sn2 (aq) + 2e- Sn(s) 0.140V Cr3 (aq) + 3e° _ Cr(s)-0.740V (1) The strongest oxidizing agent is: enter formula (2) The weakest oxidizing agent is: (3) The weakest reducing agent is: (4) The strongest reducing agent is: (5) Will F2(g) oxidize Cr(s) to Cr3 (aq)? (6) Which species can be oxidized by Sn2 (aq)? If none, leave box blank. Consider the following half-reactions:...
Consider the following half-reactions: Half-reaction E° (V) Ag+(aq) +e → Ag(s) 0.799V Cu2+(aq) + 2e →...
Consider the following half-reactions: Half-reaction E° (V) Ag+(aq) +e → Ag(s) 0.799V Cu2+(aq) + 2e → Cu(s) 0.337V Mg2+(aq) + 2e —— Mg(s) -2.370V The strongest oxidizing agent is: enter symbol The weakest oxidizing agent is: The weakest reducing agent is: The strongest reducing agent is: Will Mg(s) oxidize Ag(s) to Ag+(aq)? V Which species can be oxidized by Cu2+(aq)? If none enter none. Consider the following half-reactions: Half-reaction E° (V) 2Br (aq) 1.080V Br2(1) + 2e — Ni2+(aq) +...
Q7) Using Table 9.1 (page 294) in your textbook and/or in the slides of chapter 9...
Q7) Using Table 9.1 (page 294) in your textbook and/or in the slides of chapter 9 (online material), determine the standard free energy (AG) for the following reaction in kJ/mol. [Faraday constant = 96.5 kJ/V] [10 points) FADH2 + 1/202 - FAD + 2H+ + H:0 Show detailed calculation. Final answer without clear work will not be considered. TABLE 9.1 Standard Reduction Potentials Redox Half-Reaction 2H+ + 2e" - H a-Ketoglutarate + CO, + 2H+ 2e isocitrate NADP+ + H+...
Use the table below as the basis for the calculations needed to answer the following questions....
Use the table below as the basis for the calculations needed to answer the following questions. Standard Reduction Potentials for Redox Pairs of Biological Relevance Standard Redox Pair Number Reduction (oxidized form of reduced form) Potential, electrons Volts Acetate - pyruvate 2 -0.70 Succinate --- 2 -0.67 ketoglutarate Acetate 2 -0.60 acetaldehyde 3-phosphoglycerate glyceraldehyde-3 2 -0.55 IP arketoglutarate → 2 -0.38 isocitrate NAD+ -NADH 2 -0.32 FMN--FMNH2 2 -0.30 1,3- bisphosphoglycerate 2 -0.29 glyceraldehyde-3- IP Acetaldehyde → -0.20 ethanol Pyruvate-lactate...
Question 2 (1 point) Given the following half reactions with their corresponding standard reduction potentials, which...
Question 2 (1 point) Given the following half reactions with their corresponding standard reduction potentials, which of the following is/are true for the overall reaction happening under standard conditions? S+ 2H+ + 2e + H2S E' = -0.243 V Fe3+ + e + Fe2+ E'' - 0.771 V (CHECK THE ONE(S) THAT IS/ARE CORRECT) 1) Fe3+ has a greater affinity for electrons than S. 2) AE'O = 1.014 V for the spontaneous reaction. 3) Fe2+ is the reducing agent. 4)...
Use the table below as the basis for the calculations needed to answer the following questions,...
Use the table below as the basis for the calculations needed to answer the following questions, Standard Reduction Potentials for Redox Pairs of Biological Relevance Redox Pair (oxidized form Number of Standard Reduction reduced form) electrons Potential, Volts Acetate → pyruvate 2 -0.70 Succinate-ketoglutarate 2 -0.67 Acetate acetaldehyde 2 -0.60 3-phosphoglycerate → 2 -0.55 glyceraldehyde-3-P a-ketoglutarate isocitrate 2 -0.38 2 -0.32 2 -0.30 N -0.29 NAD+ NADH FMNFMNH2 1,3-bisphosphoglycerate → glyceraldehyde-3-P Acetaldehyde ethanol Pyruvate lactate FAD FADH2 Oxaloacetatemalate 2 -0.20...
26. Standard Reduction Potentials The standard reduc- tion potential, E", of any redox pair is defined...
26. Standard Reduction Potentials The standard reduc- tion potential, E", of any redox pair is defined for the half-cell reaction: Oxidizing agent + n electrons – reducing agent The E' values for the NAD+/NADH and pyruvate/lactate con- jugate redox pairs are -0.32 V and -0.19 V, respectively. (a) Which redox pair has the greater tendency to lose electrons? Explain. (b) Which pair is the stronger oxidizing agent? Explain. (C) Beginning with 1 M concentrations of each reactant and product at...
Answer is NOT: -0.12 Part F What is the AE, for the reduction of lactate to...
Answer is NOT: -0.12
Part F What is the AE, for the reduction of lactate to pyruvate by NAD+ under standard conditions? Express your answer using two decimal places. Templates Symbols undo regio desde keyboard shortcuts help AEG' = V Submit Request Answer Use the table below as the basis for the calculations needed to answer the following questions. Standard Reduction Potentials for Redox Pairs of Biological Relevance Standard Redox Pair Number Reduction (oxidized form of reduced form) Potential, electrons...
Question 8 Given the half-reactions and E values below, determine which species is the best reducing...
Question 8 Given the half-reactions and E values below, determine which species is the best reducing agent. MnO4 (aq) + SH+ (aq) +56 - Mn2+(aq) + 4H2O(1) E = +1.512 V 4H" (aq) +NO; (aq) + 3e - NO(g) + 2H20() E = +0.964 V Fe-(aq) + - Fe2+(5) E =+0.771 v 2H+(aq) + 2€ - H2(g) Eºr=0.000 V Он O H2 MnO4 NO, Fea-
Consider the following half-reactions: Half-reaction E° (V) 12(s) + 2e - →21"(aq) 0.535V 2H+ (aq) + 2e - → H2(g) 0.000V Cr3+(aq) + 3e —— Cr(s) -0.740V The strongest oxidizing agent is: enter formula The weakest oxidizing agent is: The weakest reducing agent is: The strongest reducing agent is: Will 12(s) reduce Cr3+(aq) to Cr(s)? — Which species can be reduced by H2(g)? If none, leave box blank. Use the References to access important values if needed for this question....
help with these please
Consider the following half-reactions: Half-reaction Eo (V) F2(g)+ 2e 2F (aq) 2.870V Sn2 (aq) + 2e- Sn(s) 0.140V Cr3 (aq) + 3e° _ Cr(s)-0.740V (1) The strongest oxidizing agent is: enter formula (2) The weakest oxidizing agent is: (3) The weakest reducing agent is: (4) The strongest reducing agent is: (5) Will F2(g) oxidize Cr(s) to Cr3 (aq)? (6) Which species can be oxidized by Sn2 (aq)? If none, leave box blank. Consider the following half-reactions:...
Consider the following half-reactions: Half-reaction E° (V) Ag+(aq) +e → Ag(s) 0.799V Cu2+(aq) + 2e → Cu(s) 0.337V Mg2+(aq) + 2e —— Mg(s) -2.370V The strongest oxidizing agent is: enter symbol The weakest oxidizing agent is: The weakest reducing agent is: The strongest reducing agent is: Will Mg(s) oxidize Ag(s) to Ag+(aq)? V Which species can be oxidized by Cu2+(aq)? If none enter none. Consider the following half-reactions: Half-reaction E° (V) 2Br (aq) 1.080V Br2(1) + 2e — Ni2+(aq) +...
Q7) Using Table 9.1 (page 294) in your textbook and/or in the slides of chapter 9 (online material), determine the standard free energy (AG) for the following reaction in kJ/mol. [Faraday constant = 96.5 kJ/V] [10 points) FADH2 + 1/202 - FAD + 2H+ + H:0 Show detailed calculation. Final answer without clear work will not be considered. TABLE 9.1 Standard Reduction Potentials Redox Half-Reaction 2H+ + 2e" - H a-Ketoglutarate + CO, + 2H+ 2e isocitrate NADP+ + H+...
Use the table below as the basis for the calculations needed to answer the following questions. Standard Reduction Potentials for Redox Pairs of Biological Relevance Standard Redox Pair Number Reduction (oxidized form of reduced form) Potential, electrons Volts Acetate - pyruvate 2 -0.70 Succinate --- 2 -0.67 ketoglutarate Acetate 2 -0.60 acetaldehyde 3-phosphoglycerate glyceraldehyde-3 2 -0.55 IP arketoglutarate → 2 -0.38 isocitrate NAD+ -NADH 2 -0.32 FMN--FMNH2 2 -0.30 1,3- bisphosphoglycerate 2 -0.29 glyceraldehyde-3- IP Acetaldehyde → -0.20 ethanol Pyruvate-lactate...
Question 2 (1 point) Given the following half reactions with their corresponding standard reduction potentials, which of the following is/are true for the overall reaction happening under standard conditions? S+ 2H+ + 2e + H2S E' = -0.243 V Fe3+ + e + Fe2+ E'' - 0.771 V (CHECK THE ONE(S) THAT IS/ARE CORRECT) 1) Fe3+ has a greater affinity for electrons than S. 2) AE'O = 1.014 V for the spontaneous reaction. 3) Fe2+ is the reducing agent. 4)...
Use the table below as the basis for the calculations needed to answer the following questions, Standard Reduction Potentials for Redox Pairs of Biological Relevance Redox Pair (oxidized form Number of Standard Reduction reduced form) electrons Potential, Volts Acetate → pyruvate 2 -0.70 Succinate-ketoglutarate 2 -0.67 Acetate acetaldehyde 2 -0.60 3-phosphoglycerate → 2 -0.55 glyceraldehyde-3-P a-ketoglutarate isocitrate 2 -0.38 2 -0.32 2 -0.30 N -0.29 NAD+ NADH FMNFMNH2 1,3-bisphosphoglycerate → glyceraldehyde-3-P Acetaldehyde ethanol Pyruvate lactate FAD FADH2 Oxaloacetatemalate 2 -0.20...
26. Standard Reduction Potentials The standard reduc- tion potential, E", of any redox pair is defined for the half-cell reaction: Oxidizing agent + n electrons – reducing agent The E' values for the NAD+/NADH and pyruvate/lactate con- jugate redox pairs are -0.32 V and -0.19 V, respectively. (a) Which redox pair has the greater tendency to lose electrons? Explain. (b) Which pair is the stronger oxidizing agent? Explain. (C) Beginning with 1 M concentrations of each reactant and product at...
Answer is NOT: -0.12
Part F What is the AE, for the reduction of lactate to pyruvate by NAD+ under standard conditions? Express your answer using two decimal places. Templates Symbols undo regio desde keyboard shortcuts help AEG' = V Submit Request Answer Use the table below as the basis for the calculations needed to answer the following questions. Standard Reduction Potentials for Redox Pairs of Biological Relevance Standard Redox Pair Number Reduction (oxidized form of reduced form) Potential, electrons...
Question 8 Given the half-reactions and E values below, determine which species is the best reducing agent. MnO4 (aq) + SH+ (aq) +56 - Mn2+(aq) + 4H2O(1) E = +1.512 V 4H" (aq) +NO; (aq) + 3e - NO(g) + 2H20() E = +0.964 V Fe-(aq) + - Fe2+(5) E =+0.771 v 2H+(aq) + 2€ - H2(g) Eºr=0.000 V Он O H2 MnO4 NO, Fea-
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