Which metal(s), if coated onto iron, would prevent the corrosion of iron? Cr, Mg or Cu?
Standard Electrode Potentials at 25 âC Reduction Half-Reaction Eâ(V) Fe2+(aq)+2eâ âFe(s) -0.45 Mg2+(aq)+2eâ âMg (s) -2.37 Cr3+(aq)+3eâ âCr (s) -0.73 Cu2+(aq)+2eâ âCu(s) 0.34
Which metal(s), if coated onto iron, would prevent the corrosion of iron? Cr, Mg or Cu?
Standard Electrode Potentials at 25 âC | |||||||||||||||
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Related questions
Calculate the equilibrium constant for each of the reactions at 25âC.
| Part A 2Fe3+(aq)+3Pb(s)â2Fe(s)+3Pb2+(aq) Express your answer using two significant figures.
Incorrect; Try Again; 4 attempts remaining Part B O2(g)+2H2O(l)+2Ni(s)â4OHâ(aq)+2Ni2+(aq) Express your answer using two significant figures.
Part C Cl2(g)+2Iâ(aq)â2Clâ(aq)+I2(s) Express your answer using two significant figures.
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Compare table 1 (the standard reduction potentials) to the periodic trends (radius, Ionization energy, electron affinity, electronegativity). Do the potentials in the table agree with our periodic trends? Why/why not (use at least two examples in your argument)?
Table 1: Standard Reduction Potentials | |
Half-Reaction | E°, volts |
Na+(aq) + eâ â Na(s) | -2.71 |
Al3+(aq) + 3 eâ â Al(s) | -1.66 |
Zn2+(aq) + 2 eâ â Zn(s) | -0.76 |
Cr3+(aq) + 3 eâ â Cr(s) | -0.74 |
Fe2+(aq) + 2 eâ â Fe(s) | -0.41 |
PbSO4(s) + 2 eâ â Pb(s) + SO42â(aq) | -0.36 |
Ni2+(aq) + 2 eâ â Ni(s) | -0.23 |
Sn2+(aq) + 2 eâ â Sn(s) | -0.14 |
Pb2+(aq) + 2 eâ â Pb(s) | -0.13 |
2 H+(aq) + 2 eâ â H2(g) | 0 |
Sn4+(aq) + 2 eâ â Sn2+(aq) | 0.15 |
AgCl(s) + eâ â Ag(s) + Clâ(aq) | 0.22 |
Cu2+(aq) + 2 eâ â Cu(s) | 0.34 |
O2(g) + 2 H2O(l) + 4 eâ â 4 OHâ(aq) | 0.4 |
H2SO3(aq) + 4 H+(aq) + 4 eâ â S(s) + 3H2O(l) | 0.45 |
Ag+(aq) + eâ â Ag(s) | 0.8 |
O2(g) + 4 H+(aq) + 4 eâ â 2 H2O(l) | 1.23 |