Given the following standard reduction potentials in acid solution:
MnO4- + 8 H+ + 5 e-® Mn+2 + 4 H2O E°cell = 1.51 V
Co+2 + 2 e-® Co E°cell = -0.28 V
Cr+3 + 3 e-® Cr E°cell = -0.74 V
The strongest oxidizing agent listed above is:
Cr3+.
Cr.
Mn2+.
Co2+.
MnO4–
Which has the highest potential?
MnO4-?
To determine the strongest oxidizing agent, we need to look at the standard reduction potentials. In general, the species with the highest reduction potential is the strongest oxidizing agent.
From the given standard reduction potentials, we can see that MnO4- has the highest reduction potential at 1.51 V. This means that MnO4- is the most likely to get reduced and gain electrons, making it a strong oxidizing agent. Therefore, the answer is MnO4-.
To find this answer, you need to compare the reduction potentials of the species given and determine which one has the highest reduction potential.