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Parts a-j of this question refer to the following cell at 298 K. Complete the diagram...

Parts a-j of this question refer to the following cell at 298 K.
Complete the diagram of the following voltaic cell:
Zinc and iron electrodes, aqueous zinc nitrate, aqueous iron (III) nitrate, potassium nitrate salt bridge.
Fe3+ (aq) + 3e- → Fe (s) E°= -0.040 V Ag+(aq) + e- → Ag(s) E°= 0.795 V
a. Identify the electrodes as Anode or Cathode. Write the correct metal for each assuming the reactions are spontaneous
b. Show the direction of the electron flow.
c. Show the movement of Fe3+, Ag+, K+ and NO3- ions
d. Write the correct half reaction under each cell and label them as reduction or oxidation half reactions

e. Write the overall balanced net ionic equation for the chemical process occurring, including states. 5
f. Calculate the Standard Potential E° for the reaction.

g. Calculate the equilibrium constant Keq for the cell at 298 K: Keq = _________________

h. Calculate the correct cell potential E (not zero) at 298 K given 0.500 M iron (III) nitrate and 0.200 M silver nitrate in the half cells.

i. Calculate ΔG° and ΔG for the cell at 298K

j. Circle the correct words:
In this cell, (electrical/chemical) energy is converted to (electrical/chemical) energy.

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Answer #1

(a)

Anode is Fe

Cathode is Ag

(b)

Electron flows from anode to cathode that Is from Irons electrode to Agree electrode.

(c)

K+ moves towards cathode

NO3- moves towards anode

Ag+ move towards electrode

Fe+3 move away from electrode

(f)

Excellent = 0.835 volt0 at Zn(s) and Fe (s) electrodes In (NO3) aqueous, Fe (NO) aqueous hjem electrolytes a thode Ak Fe(s) Cathode → Aqt moves tow

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