Why is the electrolysis of molten salts much easier to predict in terms of what occurs at the anode and cathode than the electrolysis of aqueous dissolved salts? (Select all that apply.) When H2O is present, we must consider the oxidation and reduction of water as potential reactions that can occur. There are more potential reactions when H2O is present, making predictions more difficult. There are fewer potential reactions when H2O is present, making predictions easier. When H2O is present, it is always oxidized and reduced rather than the ions of the dissolved salt. When molten salts are electrolyzed, there is only one species present that can be oxidized (the anion in simple salts), and there is only one species that can be reduced (the cation in simple salts). When molten salts are electrolyzed, there is only one species present that can be oxidized (the cation in simple salts), and there is only one species that can be reduced (the anion in simple salts).

Question

Why is the electrolysis of molten salts much easier to predict in terms of what occurs at the anode and cathode than the electrolysis of aqueous dissolved salts? (Select all that apply.)

When H2O is present, we must consider the oxidation and reduction of water as potential reactions that can occur.
There are more potential reactions when H2O is present, making predictions more difficult.
There are fewer potential reactions when H2O is present, making predictions easier.
When H2O is present, it is always oxidized and reduced rather than the ions of the dissolved salt.
When molten salts are electrolyzed, there is only one species present that can be oxidized (the anion in simple salts), and there is only one species that can be reduced (the cation in simple salts).
When molten salts are electrolyzed, there is only one species present that can be oxidized (the cation in simple salts), and there is only one species that can be reduced (the anion in simple salts).

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