The cell above uses the reaction: zn(s)+ 2Ag (aq) rightarrow zn2+ (aq) 2Ag 1. Th

Question

The cell above uses the reaction: zn(s)+ 2Ag (aq) rightarrow zn2+ (aq) 2Ag 1. The standard potential for cell above is a. 1.56V b. -0.29V C. -1.94V d. 3.66V 2. The wire ____. a. Allows ions to move between cells to keep the cells neutral b. Carries energy from one cell to the other. c. Prevents the flow of electrons. d. Carries electrons from the anode to the cathode 3. Cations ____ a. Flow through the wire from the chromium to the zinc b. Flow through the salt bridge from the zinc to the silver. c. Flow through the salt bridge from the silver to the zinc. d. Go through the wire both ways. e. Flow through the wire from the zinc to the chromium 4. The delta G degree for the reaction is ______. a. 220.0kJ b. -44.2k J C. -170.3 kJ d. -301 kJ 5. Which of the following is true for the cell above. a. The zinc electrode would get lighter. b. The K value is greater than 1 c. The silver electrode would get heavier. a. a-only b. a & c only c. a & b only d. b & c only e. a, b 8

Explanation / Answer

Q1.

For the cell

E° = Ered - Eox

Zn2+ + 2 e Zn(s) 0.7618

Ag+ + e Ag(s) +0.799

silver is reducing so

E° = Ered - Eox = 0.799 - -0.7618= 1.5608

best answer is A

Q2.

the wire carries electrons from anode to cathode

the salt bridge carries ions in order to maintian cell neutral

Q3.

cations flow from zinc to silver cathode, this is done via the salt bridge

Q4.

dG = -n*F*E°

n = 2 electrons

dG = -2*96500 * 1.5608

dG = -301234.4 J/mol

dG = -301 kJ/mol,

Q5.

a) Zinc will get lighter, sinc eit is trnasforming to Zn2+ --> TRUE

b) K> !, therefore spontaneous reaction --> TRUE

c) Ag gets heavier since Ag(s) is produced, -- >TRUE

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