Questions: How would you classify this reaction? 2 Cl2O5 -> 2 Cl2 + 5 O2 double replacement redox

Transcript text: How would you classify this reaction? \[ 2 \mathrm{Cl}_{2} \mathrm{O}_{5} \rightarrow 2 \mathrm{Cl}_{2}+5 \mathrm{O}_{2} \] double replacement redox

Solution

Solution Steps

Step 1: Identify the Reaction Type

First, we need to identify the type of chemical reaction. The given reaction is:

\[ 2 \mathrm{Cl}_{2} \mathrm{O}_{5} \rightarrow 2 \mathrm{Cl}_{2} + 5 \mathrm{O}_{2} \]

Step 2: Analyze the Reactants and Products

In this reaction, the reactant is \(\mathrm{Cl}_{2} \mathrm{O}_{5}\) and the products are \(\mathrm{Cl}_{2}\) and \(\mathrm{O}_{2}\). This indicates that a single compound is breaking down into two simpler substances.

Step 3: Determine the Reaction Classification

A reaction where a single compound breaks down into two or more simpler substances is known as a decomposition reaction. Additionally, we need to check if there is a transfer of electrons (oxidation and reduction) to classify it as a redox reaction.

Step 4: Check for Redox Characteristics

To determine if the reaction is a redox reaction, we need to check the oxidation states of the elements involved:

In \(\mathrm{Cl}_{2} \mathrm{O}_{5}\):
- Chlorine (Cl) has an oxidation state of +5.
- Oxygen (O) has an oxidation state of -2.
In \(\mathrm{Cl}_{2}\):
- Chlorine (Cl) has an oxidation state of 0.
In \(\mathrm{O}_{2}\):
- Oxygen (O) has an oxidation state of 0.