The cell above uses the reaction: Zn(s) + 2Ag^+ (aq) rightarrow Zn^2+ (aq) + 2Ag

Question

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

Explanation / Answer

Q1.

E° = Ered - Eox

E° = Eag - Ezn

E° = 0.799 - (-0.7618) = 1.56

Q2.

the wire allow selectrons to flow

Q3.

cations flow through the slat bridge, from Ag+ to Ag(s)

Q4.

dG = -nF*E

dG = -2*96500*1.56 = -301800 J = -301 kJ

Q5.

a --> true since Zn becomes ionic

b --> true sicne this is spotnaneous

c --> true since Ag is forming

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