10) Which is the oxidation half reaction for a Mg and Ag electrochemical cell? (The reaction is spontaneous.) a) Mg2 + 2e Mg(s) (Mg gains electrons) b) Mg(s) → Mg* + 2e (Mg loses electrons) c) Ag + e→ Ag (s) (Ag gains electrons) d) Ag(s) → Ag" + e (Ag loses electrons) hp

Consider the following galvanic cell:     E° (V) U3+  +  3 e−   →   U(s) −1.642 In3+  +  2e−   →   In+ −0.444 What is the anode? In3+/In+ U/U3+ Pt/In3+ Pt/In+

In the galvanic cell using the redox reaction below, the oxidation half reaction is Zn (s) + Cu2+ (aq) → Zn²+ (aq) + Cu (s) O cu2+ → Cu + 2e¯ O Cu2+ + 2e¯ → Cu O Zn → Zn2+ + 2e O Zn + 2e¯ → → Zn2+ hp Nengi Tew e i O 732006020610 fs f8 ? 米 2 6 7 8. W E R Y LO

Consider the following half-reactions.   Cl2(g) + 2 e– → 2 Cl–(aq) E° = +1.36 V   Ag+(aq) + e– → Ag(s) E° = +0.80 V   Cu2+(aq) + 2 e– → Cu(s) E° = +0.34 V   Sn2+(aq) + 2 e– → Sn(s) E° = –0.14 V   Al3+(aq) + 3 e– → Al(s) E° = –1.66 V Which of the following species will reduce Cu2+(aq) ion? Ag(s) and Sn^2+(aq) Cl^-(aq) and Ag(s) Cl2(g) and Ag^+(aq) Sn(s) and Al(s) Sn^2+(aq) and Al^3+(aq)

Consider the following standard reduction potentials in acid solution:                                E°(V) Al⁺³ + 3e− → Al(s) −1.66 Ag⁺¹ + e− → Ag(s) +0.80 Sn⁺⁴ + 2e− → Sn⁺² +0.14 Fe⁺³ + e− → Fe⁺² +0.77   The strongest reducing agent among those shown above is A) Al⁰ B) Fe⁺³ C) Br⁻ D) Al⁺³

a) Balance the following redox reaction in basic solution: H2O2(aq) + ClO2(aq) → ClO2-(aq) + O2(g) b) Sketch the voltaic cell for the redox reaction, labeling the direction for electron flow, the anode and cathode , and the species present in each half-cell. Show all the work please!

Consider the reaction: Fe(s) + CuSO4(aq) → FeSO4(aq) + Cu(s) What is the half-cell reaction for reduction? Multiple Choice О Fe(s) -> Fe2+(aq) + 2 e- Cu2+(aq) + 2 e-→ Cu(s) О Cu(s) → Cu2+(aq) + 2e- Fe(s) + 2 e-→ Fe2(aq)

Consider the following galvanic cell:     E° (V) U3+  +  3 e−   →   U(s) −1.642 In3+  +  2e−   →   In+ −0.444 The electron flow is clockwise electrons don't move in this galvanic cell counterclockwise

Calculate Ecell (volts) for the galvanic cell containing the reaction shown below where the concentration of the ion at the anode is 0.400 M and the concentration of the ion at the cathode is 1.86 M.