Question

For the following redox reaction in a galvanic cell, write the oxidation half-reaction and the reduction-half reaction, and calculate the standard cell potential of the reaction. Use Table 1 in the Background as needed. Explain how you identified which half-reaction is the oxidizer and which is the reducer. Balance the equation. Show your work. (8pts)

Al_(s) + Ag⁺¹_(aq)à Ag_(s) + Al⁺³_(aq)

_{Please type your answer out please}

Answer 1

oxidation takes place (the metal loses electrons). This is represented in the following oxidation half-reaction (note that the electrons are on the products side):

AL (s) - - - - > Al⁺³ (aq) + 3 e^- E_ox = +1.66 V ........ Eq1

reduction takes place (electrons are accepted). This is represented in the following reduction half-reaction (note that the electrons are on the reactants side):

Ag⁺¹ (aq) + 1e^- - - - - - > Ag (s) E_red = 0.8 V

Now multiply by 3 to reduction half reaction gives

3 Ag⁺¹ (aq) + 3e^- - - - - - > 3Ag (s) E_red =3 x 0.8 V = 2.4 V... eq2

Overall balanced reaction add eq1 and e2 gives

Al (s) + 3Ag⁺¹ - - - - - > 3Ag(s) + Al⁺³ (aq)

Standard cell potential E = E_ox + E_red = 1.66+2.4 =4.46 V