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I completely forgot how to figure out if a molecule is a strong or weak oxidizing agent, and how to compare them. For example, Midterm Question 7A asks to order the following oxidizing agents by increasing strength under standard state conditions: O2(g), MnO4-(aq), and NO3-(aq). How would one go about solving this? Thank you!
To solve 7A you look at the three equations, each on having one of the three oxidizing agents. You then look at the value of E knot for each equation and see which oxidizing agent resulted in the highest E knot value. The highest E knot value means the oxidizing agent is the strongest, and the lowest E knot value means the oxidizing agent is the weakest. Thus, the answer for 7A would be NO3- < O2 < MnO4-.
The E knot value given beside the options indicates their strength as an oxidizing agent, so the larger the E knot value, the stronger it is and you arrange the agents in order of increasing E knot values. :)
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