An electrochemical cell consists of a thallium electrode in a 1.00M solution of

Question

An electrochemical cell consists of a thallium electrode in a 1.00M solution of TINO3 connected by a salt bridge to a second compartment with a silver electrode in a 1.00M solution of AgNO3

a. Write the equation for the half cell reaction occurring at each electrode. Indicate which half reaction occurs at the anode

b. Write the balanced chemical equation for the overall spontaneous cell reaction that occurs when the circuit is complete. Calculate the standard voltage E^0 for this cell reaction

c. Calculate the equilibrium constant for this cell reaction at 298K

d. Of the compounds NaCl and KNO3 which one is appropriate to use a salt bridge for this cell? Explain your answer and why the other compound is not appropriate

e. Balance the following oxidation reduction reaction using the half reaction method Ag+(aq) + Mn2+(aq) -> Ag(s) + MnO4-(aq)

Explanation / Answer

a )

anode : oxidation

Ti ----------------------> Ti+2 + 2 e-   ,   Eo = -1.63 V

cathode : reduction

2Ag+ + 2e- -------------------> 2Ag   , Eo = +0.80 V

b)

overall reaction :

Ti + 2 Ag+ ----------------> Ti+2 + 2Ag

Eo = 0.80 - (-1.63) = 2.43 V

Eo = 2.43 V

c ) delta G = - n F E = - 2 x 96485 x 2.43 = -468917 J = -469 kJ

delta G = - R T ln K

-469 = - 8.314 x 10^-3 x 298 x ln K

189 = ln K

K = 1.21 x 10^82

equilibrium constant = 1.21 x 10^82

d)   KNO3 is used in salt bridge . becuase K+ and NO3- have same mobility . that means transport numbers of K+ and NO3 - are same so we used in salt bridge

e)  

balanced equation:

Mn+2 + 5 Ag+ + 4H2O ----------------> MnO4- + 8H+ + 5Ag

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