Which metals may be oxidized by H + under standard-state conditions? Ag + (aq) + e - → Ag (s) E° = 0.80 V Cu2 + (aq) + 2e - → Cu (s) E° = 0.34 V Sn2 + (aq) + 2e - → Sn (s) E° = - 0.14 V Zn2 + (aq) + 2e - → Zn (s) E° = - 0.76 V

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Chemistry

Maddison

3 January, 21:15

Which metals may be oxidized by H + under standard-state conditions? Ag + (aq) + e - → Ag (s) E° = 0.80 V Cu2 + (aq) + 2e - → Cu (s) E° = 0.34 V Sn2 + (aq) + 2e - → Sn (s) E° = - 0.14 V Zn2 + (aq) + 2e - → Zn (s) E° = - 0.76 V

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Mariah Logan · Answer 1

Answer is: tin and zinc, because they standard potential as less than zero.

Tin and zinc are oxidized to tin and zinc cations (with + 2 charge) and hydrogen anions are reduced to hydrogen molecules with neutral charge.

Zn → Zn²⁺ + 2e⁻; 2H⁺ + 2e⁻ → H₂.

Oxidation is increase of oxidation number and reduction is decrease of oxidation number.