Refer to the table of standard reduction potentials, E red, provided below. In an acidic solution, copper(I) ion is oxidized to copper(II) ion by the nitrate ion. 3Cu+(aq)+NO3(aq)+4H+(aq)NO(g)+3Cu2+(aq)+2H2O(l) Part A: Using the E red values provided, calculate the standard cell potential, E cell, (in V) for this reaction. Round your answer to TWO places past the decimal. If your answer is negative, include the sign. Ecell= Part B: Use the rounded value of E cell from Part A to calculate the standard free energy, G, (in kJ ) of the reaction at 298K Round your answer to the nearest whole number. If your answer is negative, include the sign. G= Part C: Use the rounded value of E cell from Part A to calculate the equilibrium constant, K, at 298K. Round your answer to ONE place past the decimal in scientific notation. If your answer is negative, include the sign