Question

1. The magnitudes of the standard electrode potentials of two metals, A and B, are(1) A2+ + 2e- →A |E°| = 0.63V (2) B2+ + 2e- →B |E°| = 1.24V Where the | | notation denotes that only the magnitude (but not the sign) of the E° value is shown. When half-reactions (1) and (2) are connected, electrons flow spontaneously from half-reaction (1) to half-reaction (2). When half-reaction (1) is connected to a standard hydrogen electrode (H+=H2), electrons flow spontaneously from half-reaction (1) to the standard hydrogen electrode.(a) What are the signs of E° for half-reaction (1) and half-reaction (2)?

(b) What is the standard cell potential (E°cell)of the cell made from half-reactions (1) and (2)?

1. The magnitudes of the standard electrode potentials of two metals, A and B. are (1) A2+ + 2e - A E = 0.63 V (2) B2- + 2e - B E = 1.24 V Where the notation denotes that only the magnitude (but not the sign) of the Eº value is shown. When half-reactions (1) and (2) are connected, electrons flow spontaneously from half-reaction (1) to half-reaction (2) When half-reaction (1) is connected to a standard hydrogen electrode (H* → H2), electrons flow spontaneously from half-reaction (1) to the standard hydrogen electrode. (a) What are the signs of Eº for half-reaction (1) and half-reaction (2)? (6) What is the standard cell potential (Eºcell) of the cell made from half-reactions (1) and (2)? *Hint: You have to flip one of the half reactions.