- 16 Consider The Data In The Table Shown Below Under Standard Conditions Which Of The Following Molecules Would Be Abl 1 (731.47 KiB) Viewed 78 times
16. Consider the data in the table shown below. Under standard conditions, which of the following molecules would be abl
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16. Consider the data in the table shown below. Under standard conditions, which of the following molecules would be abl
16. Consider the data in the table shown below. Under standardconditions, which of the following molecules would be able toreduce NAD+ to NADH in an energetically favorable manner?a-ketoglutarate, succinate, malate, and acetaldehyde. Explain youranswer with a sentence.
TABLE 9.1 Standard Reduction Potentials* Redox Half-Reaction 2H+ + 2e → H₂ a-Ketoglutarate + CO₂ + 2H+ + 2e¯ →isocitrate NADP+ + H+ + 2e¯ → NADPH NAD+ + H+ + 2e¯ → NADH S + 2H+ + 2e¯ → H₂S FAD + 2H+ + 2e¯ → FADH₂ Acetaldehyde + 2H+ + 2e¯ → ethanol Pyruvate + 2H+ + 2e¯ → lactate Oxaloacetate + 2H+ + 2e¯ → malate Cu²+ + e → Cu+ Fumarate + 2H+ + 2e¯ → succinate Cytochrome b (Fe³+) + e¯ → cytochrome b (Fe²+) Cytochrome c, (Fe³+) + e¯ → cytochrome c₁ (Fe²+) Cytochrome c (Fe³+) + e¯ → cytochrome c (Fe²+) Cytochrome a (Fe³+) + e¯ → cytochrome a (Fe²+) NO3 + 2H+ + 2€¯ → NO₂ + H₂O NO₂ + 8H+ + 6e¯ → NH+ + 2H₂O Fe³+ + e →→ Fe²+ ¹/2O₂ + 2H+ + 2e¯ → H₂O Standard Reduction Potentials (E°¹') (V) -0.42 -0.38 -0.324 -0.32 -0.23 -0.22 -0.20 -0.19 -0.166 +0.16 +0.031 +0.075 +0.22 +0.235 +0.29 +0.42 +0.44 +0.77 +0.82 By convention, redox reactions are written with the reducing agent to the right of the oxidizing agent and the number of electrons transferred. In this table the redox pairs are listed in order of increasing E°' values. The more negative the E°' value is for a redox pair, the lower the affinity of the oxidized component for electrons. The more positive the E°' value is, the greater the affinity of the oxidized component of the redox pair for electrons. Under appropriate conditions, la redox half-reaction reduces any of the half-reactions below it in the table. r
TABLE 9.1 Standard Reduction Potentials* Redox Half-Reaction 2H+ + 2e → H₂ a-Ketoglutarate + CO₂ + 2H+ + 2e¯ →isocitrate NADP+ + H+ + 2e¯ → NADPH NAD+ + H+ + 2e¯ → NADH S + 2H+ + 2e¯ → H₂S FAD + 2H+ + 2e¯ → FADH₂ Acetaldehyde + 2H+ + 2e¯ → ethanol Pyruvate + 2H+ + 2e¯ → lactate Oxaloacetate + 2H+ + 2e¯ → malate Cu²+ + e → Cu+ Fumarate + 2H+ + 2e¯ → succinate Cytochrome b (Fe³+) + e¯ → cytochrome b (Fe²+) Cytochrome c, (Fe³+) + e¯ → cytochrome c₁ (Fe²+) Cytochrome c (Fe³+) + e¯ → cytochrome c (Fe²+) Cytochrome a (Fe³+) + e¯ → cytochrome a (Fe²+) NO3 + 2H+ + 2€¯ → NO₂ + H₂O NO₂ + 8H+ + 6e¯ → NH+ + 2H₂O Fe³+ + e →→ Fe²+ ¹/2O₂ + 2H+ + 2e¯ → H₂O Standard Reduction Potentials (E°¹') (V) -0.42 -0.38 -0.324 -0.32 -0.23 -0.22 -0.20 -0.19 -0.166 +0.16 +0.031 +0.075 +0.22 +0.235 +0.29 +0.42 +0.44 +0.77 +0.82 By convention, redox reactions are written with the reducing agent to the right of the oxidizing agent and the number of electrons transferred. In this table the redox pairs are listed in order of increasing E°' values. The more negative the E°' value is for a redox pair, the lower the affinity of the oxidized component for electrons. The more positive the E°' value is, the greater the affinity of the oxidized component of the redox pair for electrons. Under appropriate conditions, la redox half-reaction reduces any of the half-reactions below it in the table. r