3 answers
(click or scroll down)
See your first two problems. Same solutions.
Post your work if you get stuck.
The most common method of producing bromine involves oxidizing bromine ions (Br^-) to bromine liquid (Br2) using chlorine gas (Cl2). What is the E for this reaction?
DrBob222
answered3 years ago
Step-by-Step Bot
answered1 year ago
To determine the standard reduction potential (E°) for the reaction, we need to use the standard reduction potentials for the half-reactions involved.
The reduction half-reaction for the oxidation of bromide ions (Br^-) to bromine liquid (Br2) is:
Br^- (aq) → Br2 (l) + 2e^-
The standard reduction potential for this half-reaction can be found in a table. Using the values, we find that the standard reduction potential for this half-reaction is +1.09 V.
The reduction half-reaction for the reduction of chlorine gas (Cl2) to chloride ions (Cl^-) is:
Cl2 (g) + 2e^- → 2Cl^- (aq)
The standard reduction potential for this half-reaction is +1.36 V.
To calculate the overall standard reduction potential for the reaction, we can subtract the reduction potential of the oxidation half-reaction from the reduction potential of the reduction half-reaction:
E° = (+1.36 V) - (+1.09 V)
E° = +0.27 V
Therefore, the standard reduction potential (E) for this reaction is +0.27 V.
Explain Bot
answered11 months ago
To find the standard reduction potential (E) for the given reaction, we need to look up the reduction potentials (E°) for both half-reactions involved and then apply the Nernst equation. The half-reactions involved are:
1. Oxidation half-reaction: Br^-(aq) → Br2(l) + 2e^-
2. Reduction half-reaction: Cl2(g) + 2e^- → 2Cl^-(aq)
First, let's find the E° values for these half-reactions. The reduction potentials can be found in tables or reference materials. The values at 25°C (298 K) are approximately:
E°(Br^-(aq) → Br2(l) + 2e^-) = +1.09 V
E°(Cl2(g) + 2e^- → 2Cl^-(aq)) = +1.36 V
Now, since the desired reaction involves oxidation of Br^-(aq) and reduction of Cl2(g), we need to reverse the reduction half-reaction. By doing so, we also need to change the sign of its reduction potential:
Reversed reduction half-reaction: 2Cl^-(aq) → Cl2(g) + 2e^-
E°(reversed reduction) = -E°(reduction) = -1.36 V
Now, we can write the overall balanced equation of the desired reaction:
2Br^-(aq) + Cl2(g) → Br2(l) + 2Cl^-(aq)
To calculate the overall E° for this reaction, we sum the E° values of the individual half-reaction:
E°(overall) = E°(oxidation) + E°(reversed reduction)
E°(overall) = 1.09 V + (-1.36 V)
E°(overall) = -0.27 V
Therefore, the standard reduction potential (E°) for the given reaction is approximately -0.27 V.