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Consider the following standard reduction potentials: Mnoaaq) + 8H+(aq) + 5 e-â Mn2+(aq) + 4H20(1) Eo_ +1.52 V Cd2+(aq) + 2e-â Cd(s) What is the value of E cell at 25°C for the reaction shown below? 5 Cd2+(aq) + 2 Mn2+(aq) + 8H20(1) â 5 Cd(s) + 2 Mn04-(aq) + 16H'(aq) Q7. E--0.40 V a) -1.92 v b) +1.12 V c) -5.04 V d) +1.04 V Q8. Consider the following half-reactions: Cu2+(aq) + 2e-â Cu(s) Sn2+(aq) + 2e-â Sn(s) E-+0.34% E°=-0.14 V 24 Al3+(aq) + 3 e-â Al(s) Mg2+(aq) + 2e--> Mg(s) Eo=-1.66 V Eã--2.37V Which pair of the above metals would you use as sacrificial anode to prevent iron from corroding? a) Cu (aq) and Sn2 (aq) b) Al(s) and Mg(s) c Al (aq) and Mg? (aq) d) Cu(s) and Sn(s)
Consider the following standard reduction potentials: Mnoaaq) + 8H+(aq) + 5 e-â Mn2+(aq) + 4H20(1) Eo_ +1.52 V Cd2+(aq) + 2e-â Cd(s) What is the value of E cell at 25°C for the reaction shown below? 5 Cd2+(aq) + 2 Mn2+(aq) + 8H20(1) â 5 Cd(s) + 2 Mn04-(aq) + 16H'(aq) Q7. E--0.40 V a) -1.92 v b) +1.12 V c) -5.04 V d) +1.04 V Q8. Consider the following half-reactions: Cu2+(aq) + 2e-â Cu(s) Sn2+(aq) + 2e-â Sn(s) E-+0.34% E°=-0.14 V 24 Al3+(aq) + 3 e-â Al(s) Mg2+(aq) + 2e--> Mg(s) Eo=-1.66 V Eã--2.37V Which pair of the above metals would you use as sacrificial anode to prevent iron from corroding? a) Cu (aq) and Sn2 (aq) b) Al(s) and Mg(s) c Al (aq) and Mg? (aq) d) Cu(s) and Sn(s)
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Nestor RutherfordLv2
18 Feb 2019
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