Refer to Figure 17.4 and state whether each of the following ionic redox reactions is spontaneous or nonspontaneous.

(a) Mg(s) + Sn²⁺(aq) → Mg²⁺(aq) + Sn(s)

(b) H⁺(aq) + Ni(s) → H₂(g) + Ni²⁺(aq)

Figure 17.4

 

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STRONGEST Oxidizing Agent F₂(8) Ch₂(8) Br₂(1) Ag+ (aq) Fe³+ (aq) L₂(s) Cu²+ (aq) 2 H*(aq) Pb²+ (aq) Sn²+ (aq) Ni²+ (aq) Fe²+ (aq) Cr³+ (aq) Zn²+ (aq) Mn²+ (aq) A1³+ (aq) Mg²+ (aq) Na* (aq) Ca²+(aq) K+ (aq) Li+ (aq) Weakest Oxidizing Agent +2e™ → +2e → +2e → + e→ + e → +2e → +2e →> +2e → +2e → +2e → +2e → +2e →> +3e → +2e → +2e → +3e → +2e → + e- +2e → + e- + e- Weakest Reducing Agent 2 F (aq) 2 CI (aq) 2 Br(aq) Ag(s) Fe²+ (aq) 21- (aq) Cu(s) H₂(g) Pb(s) Sn(s) Ni(s) Fe(s) Cr(s) Zn(s) Mn(s) Al(s) Mg(s) Na(s) Ca(s) K(s) Li(s) STRONGEST Reducing Agent