Au3+ (aq)+ 3e¯ E° = 1.50 V Au (s) | CIO2 (g)+ e ¯ – CIO2 E° = 0.95 V (aq) 12 (s)+ 2e- → 21° (aq) E° = 0.54 V Pb2+ (aq)+ 2e¯ E° = - 0.13 V – Pb (s) Mg2+ (aq)+ 2e¯ – Mg E° = - 2.37 V (s) Which would be the most likely to accept electrons?

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Chapter1: Chemical Foundations
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Below show several half-cell reactions and their corresponding reduction potentials.
Au3+ (aq)+ 3e¯
E° = 1.50 V
Au (s)
CIO2 (g)+ e
¯ – CIO,
E° = 0.95 V
(aq)
12 (s)+ 2e- → 21 (aq)
E° = 0.54 V
Pb2+ (aq)+ 2e¯
E° = - 0.13 V
– Pb (s)
Mg2+ (aq)+ 2e¯ – Mg
E° = - 2.37 V
(s)
Which would be the most likely to accept electrons?
O Mg2+ (aq)
Pb2* (aq)
O Au3+ (aq)
O CIO2 (g)
O 12 (s)
Transcribed Image Text:Below show several half-cell reactions and their corresponding reduction potentials. Au3+ (aq)+ 3e¯ E° = 1.50 V Au (s) CIO2 (g)+ e ¯ – CIO, E° = 0.95 V (aq) 12 (s)+ 2e- → 21 (aq) E° = 0.54 V Pb2+ (aq)+ 2e¯ E° = - 0.13 V – Pb (s) Mg2+ (aq)+ 2e¯ – Mg E° = - 2.37 V (s) Which would be the most likely to accept electrons? O Mg2+ (aq) Pb2* (aq) O Au3+ (aq) O CIO2 (g) O 12 (s)
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