Voltmeter Switch Wire Salt Bridge Sn Metal X 1.0 M Sn(NO, 10 M XINO sets up the

Question

Voltmeter Switch Wire Salt Bridge Sn Metal X 1.0 M Sn(NO, 10 M XINO sets up the electrochemical cell depicted above with the intention of the tin functioning as the anode. a) If the cell is set up so tin functions as the anode, will the mass of the tin metal increase decrease, or remain constant as the cell operates? Explain your answer. b) Based on the reduction potential above, select the metalVion pair from the choices listed in the table below that would cause the tin electrode to operate as the anode of the cell Standard Reductiorn Petential Half-Reaction EV +1.50 0.41 c) Calculate the standard cell potential, E d) The salt bridge contains aqueous sodium nitrate; which metal will the nitrate ions flow toward as the cell operales? e) A different cell is set up using 0.5 M Sn(NO>)h at the anode; the concentration of the cathode is kept 1.0 MX(NO,)h. Will the cell potential for this set-up be greater than, less than, or equal to the one depicted above? Justify your answer with an explanation.

Explanation / Answer

a. Mass decreases as the reacting anode material becomes aqueous.

b. For tin to be anode,

Sn ---> Sn+2 + 2e- , E= 0.14 V

For one of the metals to be cathode, the E(cell) should be positive for reduction and as seen from the table, the same happens for the Au (Gold) and hence, same will be used.

c. Now,

3Sn ---> 3Sn+2 + 6e- , G =-6*F*0.14

2Au+3 + 6e- ------>2Au, G = -6*F*1.50

Therefore,

3Sn + 2Au+3 ---> 3Sn+2 + 2Au, E (cell) =G1+G2/ -6*F

Therefore, E(cell)= 0.32 V.

d. In reality, anode attracts anions(negatively charged ions) because the solution around the anode accumulates (+) ions from the oxidation of the metal. Hence, the negative nitrate ions will move towards TIN (ANODE).

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