A chemist designs a galvanic cell that uses these two halfre

A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential Zn2+(aq)+2e- Zn(s) re 2103(aq)+12H+(aq)+10e- 12(s)+ 6H20( ,-+1.195 V red Answer the following questions about this cell Write a balanced equation for the half-reaction that happens at the cathode ×10 Write a balanced equation for the half-reaction that happens at the anode Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written Do you have enough information to calculate the cell voltage under standard conditions? Yes No If you said it was possible to calculate the cell voltage, do so and enter your answerV here. Round your answer to 4 significant digits.

Solution

cathode reaction

2 IO3- + 12 H+ 10 e- -> I2 + 6 H2O

anode reaction

Zn - > Zn2+ + 2 e-

Balanced reaction

for charge balance we multiply anode eqn by 5 and add both the eqn

2 IO3- + 12 H+ 5 Zn -> + 5Zn2+ I2 + 6 H2O

E = 1.195 - (-.763)

= 1.958 V (4 significant digits)

Sice Ecell >0 this is a spontaneous cell reaction.

No we do not have enough information to calculate cell potential at standard conditions as conc of active species are not mentioned.

2 KMnO₄ + 3 Zn + 4 H₂O = 2 MnO₂ + 3 Zn(OH)₂ + 2 KOH