please answer all parts to number 1. attached is the table for standard reduction potentials

1. Consider the following electrochemical cell at 25C : Fe(s)FeCl3(aq)Cl2(g)Pt a) Write each half-reaction then write the complete electrochemical reaction for this cell. Neglect any complex ion formation between Fe3+ and Clions. b) Using the table of standard reduction potentials in the text, calculate E for this cell. c) What is the equilibrium constant for the chemical reaction in part (a)? d) What is G for the chemical reaction of this cell? e) If the Cl2 pressure is 1.5bar, and the FeCl3 concentration is 0.020m, what is E for the cell? Use the Davies equation to estimate for FeCl3. Assume the Cl2 behaves as an ideal gas. f) Which direction will electrons spontaneously flow if the Fe terminal is connected to the Pt at the conditions of part(e)? Table 6D.1 Standard potentials at 298K. (b) In alphabetical order E/V+0.52+0.34+0.16+2.870.440.04+0.77+0.360,bydefinition0.83+1.60+1.63+1.78+3.0+0.79+0.27+0.86+0.92+0.62+0.54+0.530.140.400.440.340.492.932.523.052.361.18 Table 6D.1 (Continued)