Chapter 19, Problem 19.149MP

Consider a galvanic cell that uses the following half-reactions:
$\begin{array}{l}2H^{+}(aq)+2e^{-}\to H_2(g)\\ A{l}^{3+}(aq)+3e^{-}\to Al(s)\end{array}$
a) What materials are used for the electrodes? Identify the anode and cathode, and indicate the direction of electron and ion flow.
(b) Write a balanced equation for the cell reaction, and calculate the standard cell potential.
(c) Calculate the cell poential at 25 °C if the iOflconcentrad ons are 0.10 M and the partial pressure of H, is 10.0 atm.
(d) Calculate $\Delta G^o$ (in kilojoules) and K for the cell reaction at 25 °C.
(e) Calculate the mass change (in grams) of the aluminum electrode after the cell has supplied a constant current of 10.0 A for 25.0 mm.