An electrochemical cell based on the decomposition of H2O2 can be constructed based on the half-reactions in the table below.
Half-Reaction | Standard Reduction Potential, E°
H2O2+ 2e- => 2 OH- | 0.88 V
O2+ 2 H2O + 2e- => H2O + 2 OH- | -0.15 V
(d) Calculate the value of the standard cell potential, E °, for the cell.
(e) Indicate whether ΔG° for the decomposition reaction is greater than 0, less than 0, or equal to 0. Justify your answer.
(f) The decomposition of H2O2(aq) is slow at 298 K, but a suitable catalyst greatly increases the rate of the decomposition reaction.
(i) Draw a circle around each of the quantities below that has a different value for the catalyzed reaction than for the uncatalyzed reaction.
Keq DeltaG° DeltaH° Ea
(ii) For any quantity that you circled above, indicate whether its value is greater or less for the catalyzed reaction than for the uncatalyzed reaction. Explain why.
posted by Anonymous