Complete the following equation. Using Table 15.2, predict whether you would expect the reaction to occur to any significant extent or whether the reaction is more likely to occur in the opposite direction.
HSO4 (aq) + CIO-(aq) →
The Correct Answer and Explanation is :
To answer your question, I’ll need to look into the specific chemical reaction and determine the direction in which it is most likely to proceed, based on the principles of redox chemistry and Table 15.2, which typically contains standard reduction potentials for various half-reactions.
The reaction you’ve provided:
[
HSO_4^- (aq) + ClO^-(aq) \rightarrow ?
]
is likely to involve an oxidation-reduction (redox) process where one of the species is oxidized, and the other is reduced.
Predicting the Reaction Direction:
- Reduction Potentials (Table 15.2):
From standard reduction potentials, we can assess which species is more likely to gain electrons (reduced) and which is more likely to lose electrons (oxidized).
- The bisulfate ion (HSO4^-) can act as an oxidizing agent, and it has a standard reduction potential that indicates it might be reduced to sulfurous acid (H2SO3).
- The hypochlorite ion (ClO^-) is a strong oxidizing agent and can be reduced to chloride (Cl-) under the right conditions. Based on the standard reduction potentials for these species, the hypochlorite ion (ClO^-) will likely be reduced to chloride (Cl-), while the bisulfate ion (HSO4^-) will be oxidized.
- Direction of the Reaction:
The reaction will occur in the forward direction, as hypochlorite (ClO^-) will accept electrons and get reduced, while HSO4^- will lose electrons and be oxidized. The overall reaction could look something like this:
[
HSO_4^- (aq) + ClO^-(aq) \rightarrow H2SO3 (aq) + Cl^-(aq)
]
This is based on the principle that reactions tend to proceed in the direction where the overall Gibbs free energy change is negative, favoring the reduction of the stronger oxidizing agent (ClO^-).
Conclusion:
Using Table 15.2 to determine the standard reduction potentials, the reaction is more likely to proceed in the forward direction, where ClO^- is reduced to chloride (Cl^-) and HSO4^- is oxidized to sulfurous acid (H2SO3).
I’ll now generate the corresponding image of the reaction if you’d like to visualize it. Let me know if you’d like that!