Consider a galvanic cell at T = 298K. F = 96 485C. At the beginning (t0), [Ca2+] = 0.01M, [H+] = 1M, [HfO2+] = 2M. Consider the half-reactions below: Ca2+(aq) + 2e- → Ca(s) E0red = - 2.76 V HfO2+(aq) + 2H+(aq) + 4e- → Hf(s) + H2O(l) E0red = -1.72 V a. Find the general reaction, E0cell, and identify the cathode and the anode. Indicate the direction of the flow of electrons (from which solid plate to the other solid plate). b. Write the line notation for this cell. c. Find ΔG0.
Consider a galvanic cell at T = 298K. F = 96 485C.
At the beginning (t0), [Ca2+] = 0.01M, [H+] = 1M, [HfO2+] = 2M.
Consider the half-reactions below:
Ca2+(aq) + 2e- → Ca(s) E0red = - 2.76 V
HfO2+(aq) + 2H+(aq) + 4e- → Hf(s) + H2O(l) E0red = -1.72 V
a. Find the general reaction, E0cell, and identify the cathode and the anode. Indicate the direction of the flow of electrons (from which solid plate to the other solid plate).
b. Write the line notation for this cell.
c. Find ΔG0.
*d. Express and calculate Q (at t0)
e. Express and calculate K.
f. What value do you expect for Ecell at this point? Why?
g. Find Ecell (at t0)
After a certain period of time (t1), the H+ concentration is one-fifth of its initial concentration.
*h. Do the RICE and find the concentrations of all species at t1
i. Find the pH at t1 in two different ways.
*¥j. If no other species were in solution, what could be the pH and the concentration of H+at equilibrium? (No calculations needed)
*¥k. If we were to redo the experiment at 310K. Would Ecell be larger, smaller or equal (than Ecell in the above situation) at t0, t1 and at equilibrium? (No calculations needed)
* : Independent of the above questions
¥ : More difficult question
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