Question
Referring to Figure 21.6, would you expect $\mathrm{H}_2 \mathrm{O}$ and $\mathrm{H}^{+}$to be reduced at the cathode and $\mathrm{H}_2 \mathrm{O}$ oxidized at the anode?
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Referring to Figure $21.6,$ would you expect $\mathrm{H}_{2} \mathrm{O}$ and $\mathrm{H}^{+}$ to be reduced at the cathode and $\mathrm{H}_{2} \mathrm{O}$ oxidized at the anode?
Referring to Figure $23.6,$ would you expect $\mathrm{H}_{2} \mathrm{O}$ and $\mathrm{H}$ to be reduced at the cathode and $\mathrm{H}_{2} \mathrm{O}$ oxidized at the anode?
The apparatus in Figure $\mathrm{P} 17.7$ is used for the electrolysis of water. Hydrogen and oxygen gas are collected in the two inverted burets. An inert electrode at the bottom of the left buret is connected to the negative terminal of a 6 -volt battery; the electrode in the buret on the right is connected to the positive terminal. A small quantity of sulfuric acid is added to speed up the electrolytic reaction. a. What are the half-reactions at the left and right electrodes and their standard potentials? b. Why does sulfuric acid make the electrolysis reaction go more rapidly? (FIGURE CANNOT COPY)
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