Answer the following three questions regarding the voltaic cell shown at the rig

Question

Answer the following three questions regarding the voltaic cell shown at the right. The cell has a zinc (Zn) electrode in a zinc nitrate ( Zn(NOs)z ) solution and a copper (Cu) electrode in a copper sulfate (CuSO) solution. The salt bridge contains potassium chloride (KCI) solution. Note that direction of electron flow is shown with arrows NO, Cu NO, so, NO, NO 8. The overall reaction that takes place in the cell above is- Which ONE of the following statements is true concerning the voltaic cell above ? 9. A) 8) The Cu anode mass decreases as the cell discharges C) The Cu anode mass increases as the cell discharges. D) E) The mass of the Cu electrode does not change as the cell discharges The Cu cathode mass increases as the cell discharges. The Cu cathode mass decreases as the cell discharges. 10. Which ONE of the following statements is true concerning the half-cell on the left with the zinc electrode as the voltaic cell discharges? A) ?Zn, decreases with time, and [Cr] increases with time. B) IZn21 increases with time, and [CF] increases with time. C) [Zn2] decreases with time, and [Cr] decreases with time. D) IZn2] decreases with time, and [NO,1 increases with time. E) [Zn2] increases with time, and [NO,1 increases with time. An electrochemical cell is constructed from half cells in which the half reactions shown above take place. What is the balanced spontaneous reaction and standard cell potential of this cell? B) Pbis)+Zn2(aa)->Pb2 (aq)Znis -0.633 V C) Pb(aq) Zn2 (aq)PbsZn(s); 0.893 V E) Pbis)+ Zn2(aq) Pb* (oa)+Zn/s);-0.317 V 12. Given: Zn2 (aq) + 2eZn(s); -0.76 V 2(s)+2e2(aq); E 0.54 V 2H.(aq) + 2e > H2(g); E?= 0.00 V Bra()+ 2e2 Br(aq); E 1.07 V Cu"(aq) + 2e--> Cu(s); E. 0.34 V Which ONE of the following species will oxidize Ni but not Cu? A) Zn2 B) Br C) H D) l2 E) Zn

Explanation / Answer

8.

(D) Zn (s) + Cu2+ (aq.) ---------> Zn2+ (aq.) + Cu (s)

9.

(A) Copper cathode mass increases

10.

(B) [Zn2+] increases with time and [Cl-] increases with time

11.

(A)

Pb2+ (aq.) + Zn (s) ---------> Pb (s) + Zn2+ (aq.)

E0cell = E0Pb2+/Pb - E0Zn2+/Zn = - 0.133 - ( - 0.763 ) = + 0.633 V

12.

(C) H+

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.