d) The value of the standard cell potential, E°, for the cell is 0.73 V.
e) ΔG° for the decomposition reaction is less than 0, because the reaction is spontaneous.
f) (i) Keq, DeltaG°, and Ea have different values for the catalyzed reaction than for the uncatalyzed reaction.
(ii) The values of Keq, DeltaG°, and Ea are all greater for the catalyzed reaction than for the uncatalyzed reaction. This is because the catalyst increases the rate of the reaction, making it more favorable and thus increasing the value of these quantities.
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.
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