Which of the following statements is/are correct about the reaction.
`4CrO_(5)+6H_(2)SO_(4)to2Cr_(2)(SO_(4))_(3)+6H_(2)O+7O_(2)`

Options

A. It is disproportionation reaction.
B. It is a an intramolecular redox reaction.
C. Cr acts as an oxidant, whereas O acts as a reductant.
D. `CrO_(5)` acts as-oxidant and reductant both.

Explanation

To analyze the reaction \(4CrO_5 + 6H_2SO_4 \rightarrow 2Cr_2(SO_4)_3 + 6H_2O + 7O_2\) and determine which statements are correct, we can follow these steps:

### Step 1: Determine the oxidation states of chromium in \(CrO_5\) and \(Cr_2(SO_4)_3\)

1. **For \(CrO_5\)**:
- Let the oxidation state of chromium be \(x\).
- The oxidation state of oxygen is \(-2\).
- The equation for the oxidation states is:
\[ x + 5(-2) = 0 \implies x - 10 = 0 \implies x = +10 \]
- However, chromium can only have a maximum oxidation state of +6. In \(CrO_5\), the structure is such that 4 of the oxygen atoms are in a -1 state, and 1 is in a -2 state, which gives:
\[ x + 4(-1) + (-2) = 0 \implies x - 4 - 2 = 0 \implies x = +6 \]

2. **For \(Cr_2(SO_4)_3\)**:
- Each sulfate ion \(SO_4^{2-}\) has a -2 charge.
- Let the oxidation state of chromium in \(Cr_2(SO_4)_3\) be \(y\).
- The equation for the oxidation states is:
\[ 2y + 3(-2) = 0 \implies 2y - 6 = 0 \implies 2y = 6 \implies y = +3 \]

### Step 2: Analyze the changes in oxidation states

- In the reaction, chromium changes from +6 in \(CrO_5\) to +3 in \(Cr_2(SO_4)_3\). This indicates a reduction (gain of electrons).
- The oxygen in \(CrO_5\) is converted to \(O_2\) (where the oxidation state is 0), indicating that oxygen is undergoing oxidation (loss of electrons).

### Step 3: Classify the type of reaction

- Since \(CrO_5\) contains both oxidation and reduction processes occurring simultaneously, this reaction is classified as an **intramolecular redox reaction**. It is not a disproportionation reaction because it does not involve a single species converting to two different oxidation states.

### Step 4: Identify the oxidizing and reducing agents

- \(CrO_5\) acts as an oxidizing agent because it contains chromium in a higher oxidation state (+6) that gets reduced.
- Oxygen acts as a reducing agent because it is being oxidized from -2 in \(CrO_5\) to 0 in \(O_2\).

### Conclusion

Based on the analysis:
- The oxidation state of chromium changes from +6 to +3 (reduction).
- Oxygen changes from -2 to 0 (oxidation).
- The reaction is an intramolecular redox reaction.
- \(CrO_5\) acts as both an oxidizing agent and a reducing agent.

### Summary of Correct Statements
1. Chromium in \(CrO_5\) is reduced from +6 to +3.
2. Oxygen in \(CrO_5\) is oxidized to \(O_2\).
3. The reaction is an intramolecular redox reaction.
4. \(CrO_5\) acts as both an oxidizing agent and a reducing agent.