Understanding the Standard Reduction Potential Chart The standard reduction potentialis 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- → H2(g)has been assigned a value of 0.00 Vand all other species are compared to H+(aq)in their tendency to be reduced. So, when we see the reaction: F2(g)+ 2 e- → 2 F–(aq)has a reduction potential of 2.87 V, we can say that F2(g)is much morelikely 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 lesslikely to be reduced than H+(aq).
ChemistryPOGIL – Standard Reduction PotentialsMs. Park8. Looking at the E°redchart, circle the species that is more likely to be reduced. Explain your reasoning with #’s as evidence. a) Cu2+(aq)or Ag+(aq)b) Cl2(g)or Br2(l)9. Define oxidizing agent. 10. Circle the species that is a better oxidizing agent? Explain your reasoning.(#’s) a) Cu2+(aq)or Ag+(aq)b) MnO4–(aq)or Cr2O72–(aq)11. On your standard reduction potential table, highlight the top ten oxidizing agents(not the whole equation).