Which of the following statements is true concerning half-cell I as the voltaic

Question

Which of the following statements is true concerning half-cell I as the voltaic cell shown below discharges? a. [Zn^2+] increases with time, and [Cl] increases with time. b. [Zn^2+] decreases with time, and [Cl^-] increases with time. c. [Zn^2+] decreases with time and [Cl^-] decreases with time. d. [Zn^2+] decreases with time, and [NO_3^-] increases with time. e. [Zn^2+] increases with time, and [NO_3^-] increases with time. According to the following cell notation, which species is undergoing reduction? Sn | Sn^2+(aq) || Mn^2+ (aq) | MnO_2(s) | Pt(s) a. Mn^2+ (aq) b. Sn^2+(aq) c. Sn(s) d. MnO_2(s) e. Pt(s) In the following electrochemical cell, what is the reduction half reaction? Mn(s) | Mn^2+(aq) || Fe^3+ (aq), Fe^2+(aq) | Pt(s) a. Fe^3+(aq) + e rightarrow Fe^2+ (aq) b. Fe^2+(aq) + e rightarrow Fe^3+(aq) c. Fe^2+(aq) + Pt(s) rightarrow Fe^3+(aq) + e d. Mn^2+(aq) rightarrow Mn(s) + 2e^- e. Mn(s) rightarrow Mn^2+ (aq) + 2e^-

Explanation / Answer

(12)

(a)

Because at anode Zn metal undergoes oxidation forming Zn2+ ion which enters into the solution of anode compartment. So, the concentration of Zn2+ wll be increased with time.

At the same time to maintain electrical nutrality, Cl- ions enter into the anode compartment from salt bridge, to balance extra Zn2+ ions. Hence the concentration of Cl- ions also increases.

(13) (d) MnO2 undergoes reduction ot Mn2+.

Because, E0MnO2/Mn2+ = + 1.224 V is geater than E0Sn2+/Sn = - 0.138

(14) (a) The right part of the cell notation indicates the reduction half reaction.

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