Macmillan Learning Calculate the standard potential, E, for this reaction from its equilibrium constant at 298 K. X(s) + Y4 (aq) = X¹ (aq) + Y(s) K = 4.84 x 10-7 E 11 -0.0355 Incorrect

Table 17-1 lists common half-reactions along with the standard reduction potential associated with each half-reaction. These standard reduction potentials are all relative to some standard. What is the standard (zero point)? lf is positive for a half-reaction, what does it mean? If is negative for a half-reaction, what does it mean? Which species in Table 17-1 is most easily reduced? Least easily reduced? The reverse of the half-reactions in Table 17-1 are the oxidation half-reactions. How are standard oxidation potentials determined? In Table 17-1, which species is the best reducing agent? The worst reducing agent? To determine the standard cell potential for a redox reaction, the standard reduction potential is added to the standard oxidation potential. What must be true about this sum if the cell is to be spontaneous (produce a galvanic cell)? Standard reduction and oxidation potentials are intensive. What does this mean? Summarize how line notation is used to describe galvanic cells.

Calculate K at 25°C for each of the reactions referred to in Question 32. Assume smallest whole-number coefficients.

Calculate G and K at 25C for the reactions in Exercises 37 and 41.