Given the reaction: MnO_2(s) + H_3AsO_3(aq) + 2H^+(aq) rightarrow H_3AsO_4(aq) +

Question

Given the reaction: MnO_2(s) + H_3AsO_3(aq) + 2H^+(aq) rightarrow H_3AsO_4(aq) + Mn^2+(aq) + H_2O(l) a- Write each half reaction: b. What reaction occurs at the cathode and which at the anode? c. Which way are the electrons moving? What way are the ions moving (be specific each one) d. What is the standard emf for the cell? e. If the reaction was carried out at 298K and (MnO_2) = 2M, [H_3ASO_3] = 1M, [H^+] = 3M, [H_3AsO_4] = .5M and the [Mn^2+] = 2.3M, what is the emf for the cell? Using the concentrations from e) except for the H+, and if I told you that the emf for the cell was .55 volts what is the pH of the reaction? What is the equilibrium constant K for the reaction.

Explanation / Answer

everythig superb . small correction in (b). you have to write complete half reactions at each electrode

b)

reaction occur at anode : oxidation :

H3AsO3 + H2O ---------------------> H3AsO4 + 2H+ + e-

reaction occur at cathode : reduction

MnO2   + 4H+   + 3e- ------------------> Mn+2 + 2H2O  

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