The oxidizing agent in the reaction, 3Br\(_2\) + 6OH\(^-\) \(\rightarrow\) BrO\(_3^-\) + 5Br\(^-\) + 3H\(_2\)O...
The oxidizing agent in the reaction, 3Br\(_2\) + 6OH\(^-\) \(\rightarrow\) BrO\(_3^-\) + 5Br\(^-\) + 3H\(_2\)O is _______
- A)Br\(_2\)
- B)OH\(^-\)
- C)BrO\(_3^-\)
- D)e\(^-\)
Correct Answer: A)Br\(_2\)
Explanation
An oxidizing agent is a substance that gains electrons and causes another substance to be oxidized in a chemical reaction. In the given reaction:
\(3Br_2 + 6OH^- \rightarrow BrO_3^- + 5Br^- + 3H_2O\)
To identify the oxidizing agent, we first need to determine the oxidation states of the elements in the reactants and products. Here are the oxidation states:
Bromine (Br):
- In \(Br_2\): 0 (elementary state)
- In \(BrO_3^-\): +5 (Br is bonded to three oxygen atoms, and oxygen has an oxidation state of -2)
- In \(Br^-\): -1 (bromine has gained an electron)
Hydroxide (OH):
- In \(OH^-\): -1 (oxygen has an oxidation state of -2, and hydrogen has an oxidation state of +1)
Comparing the oxidation states, we can see that bromine in \(Br_2\) has increased its oxidation state from 0 to +5 in \(BrO_3^-\) and to -1 in \(Br^-\). This means that \(Br_2\) has lost electrons during the reaction, making it the oxidizing agent.
So, the correct answer isOption A: Br\(_2\).