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A galvanic cell is powered by the following redox reaction: (aq) (aq) (aq)(s) (l) (l) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. Write a balanced equation for the half-reaction that takes place at the cathode. Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. Round your answer to decimal places.

Respuesta :

Answer:

The redox reaction in the question is missing. The reaction is :

Cl 2(g) + Mn 2 +(aq) + 2 H-On â 2 Cl-(aq) + MnO2(s) + 4 H + (aq)

2.59V

Explanation:

A redox reaction is also known as oxidation - reduction reaction. In redox reaction, there is a transfer of electrons between the species. In one species there is oxidation and in the other species there is reduction process.

Cathode half reaction equation:

[tex]$ Cl_2(aq) + 2e \rightarrow 2Cl^- (aq)$[/tex]

Anode half reaction equation:

[tex]$ Mn^2 (aq) + 2H_2O (l) \rightarrow MnO_2 (s) +2e +4H[/tex]

E°cathode= 1.36V

E°anode= -1.23V

E°cell= E°cathode - E°anode

E°cell= 1.36 - (-1.23)

E°cell= 2.59V

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