How would each of the following change the rate of the reaction shown here?
Drag the appropriate items to their respective bins.
Li+ (aq) + Ie-→Li(s)
Fe3+ (aq) + 3e- →Fe (s)
Kt (aq) + e-→K(s)
Ni(s)→Ni2+(aq) +2e-
Increasing the concentration of Li+ (aq):
- Increase the rate of the reaction
Increasing the concentration of Fe3+ (aq):
- Increase the rate of the reaction
Increasing the concentration of Kt (aq):
- Increase the rate of the reaction
Increasing the concentration of Ni(s):
- No effect on the rate of the reaction.
To determine how each of the following would change the rate of the given reaction, let's analyze each case separately:
1. Li+ (aq) + I- → Li(s)
- Adding Li+ ions (Li+) to the reaction mixture would increase the concentration of the reactant, which would increase the rate of the reaction.
2. Fe3+ (aq) + 3e- → Fe(s)
- Adding Fe3+ ions (Fe3+) to the reaction mixture would increase the concentration of the reactant, which would increase the rate of the reaction.
3. K+ (aq) + e- → K(s)
- Adding K+ ions (K+) to the reaction mixture would increase the concentration of the reactant, which would increase the rate of the reaction.
4. Ni(s) → Ni2+ (aq) + 2e-
- Removing Ni(s) (solid nickel) from the reaction and replacing it with Ni2+ ions (Ni2+) would decrease the concentration of the reactant, which would decrease the rate of the reaction.
Therefore, the changes in the rate of the reaction based on the given cases are as follows:
- Adding Li+ ions, Fe3+ ions, and K+ ions would increase the rate.
- Replacing Ni(s) with Ni2+ ions would decrease the rate.
To determine how each of the following species would change the rate of the given reaction, we need to consider their role as oxidizing agents or reducing agents.
Oxidizing agents are substances that gain electrons during a redox reaction and are typically reduced. Reducing agents, on the other hand, are substances that lose electrons during a redox reaction and are typically oxidized.
Let's analyze each of the species mentioned in the question:
Li+ (aq) + Ie- → Li(s)
- Li+ (aq) is a cation and acts as an oxidizing agent since it accepts an electron (Ie-) during this reduction half-reaction. Its presence as an oxidizing agent would increase the rate of the reaction.
Fe3+ (aq) + 3e- → Fe (s)
- Fe3+ (aq) is also a cation and acts as an oxidizing agent as it gains three electrons during this reduction half-reaction. In this case, the presence of Fe3+ (aq) as an oxidizing agent would increase the rate of the reaction.
Kt (aq) + e- → K(s)
- Kt (aq) is an anion and therefore acts as a reducing agent since it loses an electron (e-) during this oxidation half-reaction. Its presence as a reducing agent would decrease the rate of the reaction.
Ni(s) → Ni2+ (aq) + 2e-
- Ni(s) is a solid metal and is being oxidized in this reaction since it is losing two electrons. Therefore, its presence as a reducing agent would decrease the rate of the reaction.
In summary:
- Li+ (aq) and Fe3+ (aq) act as oxidizing agents, increasing the rate of the reaction.
- Kt (aq) acts as a reducing agent, decreasing the rate of the reaction.
- Ni(s) acts as a reducing agent, decreasing the rate of the reaction.