Worksheet: Standard Reduction Potential

In this worksheet, we will practice using standard reduction potentials to identify the reduction and oxidation reactions in an electrochemical process.

Q1:

Using the standard electrode potentials shown in the table, determine which of the following metals is the most prone to corrosion.

Half-EquationAu()+3eAu()3+aqsFe()+2eFe()2+aqsFe()+eFe()3+2+aqaqMg()+2eMg()2+aqsHg()+2e2Hg()22+aqlHg()+2eHg()2+aqlZn()+2eZn()2+aqs
Standard Electrode Potential, 𝐸(V)+1.4980.447+0.7712.372+0.7973+0.8510.7618
  • AZn
  • BMg
  • CFe
  • DAu
  • EHg

Q2:

Using the standard electrode potentials shown in the table, determine which of the following ions is the strongest oxidizing agent in acidic aqueous solutions.

Half-EquationCrO+14H+6e2Cr+7HO272+3+2MnO+8H+5eMn+4HO4+2+2TiO+4H+2eTi+2HO2+2+2
Standard Electrode Potential, 𝐸(V)+1.33+1.510.50
  • AChromium(III) ions
  • BTitanium dioxide, which contains titanium(IV)
  • CDichromate ions, which contain chromium(VI)
  • DPermanganate ions, which contain manganese(VII)
  • EManganese(II) ions

Q3:

Iron, the major reactive component of steel, has a standard reduction potential of 0.447 V. Using the standard electrode potentials shown in the table, determine which of the following metals could be used as a sacrificial anode in the cathodic protection of an underground steel storage tank.

Half-EquationCd()+2eCd()2+aqsAu()+3eAu()3+aqsNi()+2eNi()2+aqsAg()+eAg()+aqsZn()+2eZn()2+aqs
Standard Electrode Potential, 𝐸 (V)0.4030+1.4980.257+0.79960.7618
  • ACd
  • BAg
  • CAu
  • DZn
  • ENi

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