Understanding the Standard Reduction Potential Chart The standard reduction

Understanding the standard reduction potential chart

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Understanding the Standard Reduction Potential Chart The standard reduction potential is the tendency for a chemical species to be reduced , and is measured in volts at standard conditions. The more positive the potential is the more likely it will be reduced . The standard potentials are all measured at standard conditions , which in electrochemistry are 298 K, 1 atm, and with 1 M solutions . Oxidation and reduction occur together . We cannot measure a reduction potential alone so a reference point is needed. That reference point is the standard hydrogen electrode (SHE) . The reaction: 2 H + (aq) + 2 e- H 2 (g) has been assigned a value of 0.00 V and all other species are compared to H + (aq) in their tendency to be reduced . So, when we see the reaction: F 2 (g) + 2 e- 2 F (aq) has a reduction potential of 2.87 V , we can say that F 2 (g) is much more likely to be reduced than H + (aq) . When we see the reaction: Li + (aq) + e- Li (s) with a reduction potential of –3.05 V , we can say that Li + is much less likely to be reduced than H + (aq) .
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Chemistry POGIL – Standard Reduction Potentials Ms. Park 8. Looking at the E° red chart, circle the species that is more likely to be reduced. Explain your reasoning with #’s as evidence. a) Cu 2+ (aq) or Ag + (aq) b) Cl 2 (g) or Br 2 (l) 9. Define oxidizing agent. 10. Circle the species that is a better oxidizing agent? Explain your reasoning.(#’s) a) Cu 2+ (aq) or Ag + (aq) b) MnO 4 (aq) or Cr 2 O 7 2– (aq) 11. On your standard reduction potential table, highlight the top ten oxidizing agents (not the whole equation).
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