What is the oxidizing agent in the following reaction?
Cl2 (g) + 2Na+ (aq) + 2Br- (aq) --> 2Na+ (aq) + 2Cl- (aq) + Br2 (l)
To determine the oxidizing agent in a reaction, we need to identify the species that is being reduced. In this reaction, we can see that Cl2 is being reduced to Cl- ions, while Br- ions are being oxidized to Br2.
To understand this, let's break down the reaction:
Cl2 (g) + 2Na+ (aq) + 2Br- (aq) --> 2Na+ (aq) + 2Cl- (aq) + Br2 (l)
In this reaction, Cl2 gains electrons (reduction) to form Cl- ions, changing its oxidation state from 0 to -1. On the other hand, Br- loses electrons (oxidation) to form Br2, changing its oxidation state from -1 to 0.
Remember, the oxidizing agent is the species that is causing another species to be oxidized. In this reaction, Br- is being oxidized, so Cl2 is the oxidizing agent.
To verify this, you can look at the changes in oxidation states of the species involved in the reaction. In this case, Cl2 is reducing from 0 to -1, indicating the transfer of electrons from Cl2 to Br-, which supports the identification of Cl2 as the oxidizing agent.
Therefore, the oxidizing agent in this reaction is Cl2.
To determine the oxidizing agent in the given reaction, we need to compare the oxidation states of the elements before and after the reaction.
In the reaction:
Cl2 (g) + 2Na+ (aq) + 2Br- (aq) --> 2Na+ (aq) + 2Cl- (aq) + Br2 (l)
Let's calculate the oxidation states of chlorine and bromine in the reactants and products:
In Cl2 (g), each Cl atom has an oxidation state of 0.
In 2Na+ (aq), each Na ion has an oxidation state of +1.
In 2Br- (aq), each Br ion has an oxidation state of -1.
In 2Na+ (aq), each Na ion has an oxidation state of +1.
In 2Cl- (aq), each Cl ion has an oxidation state of -1.
In Br2 (l), each Br atom has an oxidation state of 0.
By comparing the oxidation states of chlorine and bromine, we can see that chlorine is reduced from an oxidation state of 0 to -1, while bromine is oxidized from an oxidation state of -1 to 0.
Therefore, bromine is the oxidizing agent in the given reaction.
Oxidation is the loss of electrons.
Reduction is gain of electrons.
Substance oxidized is reducing agent.
Substance reduced is oxidizing agent.