am having trouble understanding this redox rxn.....tell me if i classify it correctly...
2K + Cl2---> 2KCl
oxidized is Cl is the recducing agent
reduced is K is the oxidizing agent
K goes from 0 oxidation state on left to +1 on the right. That is a loss of electrons which makes it oxidized and the reducing agent. Cl2 is the reverse.
To classify the redox reaction correctly, you need to identify the species that undergoes oxidation and reduction. Here's how you can analyze the reaction:
1. Identify the oxidation number of each element in the reactants and products.
- In this case, potassium (K) has an oxidation number of 0 since it is in its elemental form.
- Chlorine (Cl) has an oxidation number of 0 because it is also in its elemental form.
- In potassium chloride (KCl), potassium has an oxidation number of +1, while chlorine has an oxidation number of -1.
2. Compare the oxidation numbers of each element before and after the reaction.
- In the reactants, both K and Cl have oxidation numbers of 0.
- In the products, K has an oxidation number of +1, while Cl has an oxidation number of -1.
Based on the changes in oxidation numbers, you can classify the reaction as follows:
- The element that undergoes oxidation is chlorine (Cl). Its oxidation number changes from 0 to -1, indicating the loss of electrons. Therefore, chlorine is the reducing agent because it causes another species to be reduced.
- The element that undergoes reduction is potassium (K). Its oxidation number changes from 0 to +1, indicating the gain of electrons. Therefore, potassium is the oxidizing agent because it causes another species to be oxidized.
So, your classification is correct:
Oxidized: Chlorine (Cl), reducing agent
Reduced: Potassium (K), oxidizing agent