With reference to the chemical reaction
`K_2 Cr_2O_7 + 14HCl to 2KCl + 2CrCl_3 + 3Cl_2 + ` Consider the following statements
1. `K_2Cr_2O_7` acts as oxidising agent.
2. HCl is the reducing agent.
3. `K_2Cr_2O_7` is the reducing agent.
4. HCl is the oxidising agent.
Which of the following statements are correct?

Options

A. 1 and 2
B. 2 and 3
C. 1 and 4
D. 2 and 4

Explanation

To analyze the given chemical reaction and determine the correctness of the statements, we will follow these steps:

### Step 1: Identify the Reactants and Products
The reaction given is:
\[ K_2Cr_2O_7 + 14HCl \rightarrow 2KCl + 2CrCl_3 + 3Cl_2 + 7H_2O \]

### Step 2: Determine Oxidation States
- **Potassium Dichromate (\(K_2Cr_2O_7\))**:
- The oxidation state of chromium (Cr) in \(K_2Cr_2O_7\) is +6.
- **Chromium Chloride (\(CrCl_3\))**:
- The oxidation state of chromium (Cr) in \(CrCl_3\) is +3.

### Step 3: Analyze Changes in Oxidation States
- The change in oxidation state for chromium is from +6 in \(K_2Cr_2O_7\) to +3 in \(CrCl_3\). This indicates that chromium is being reduced (gaining electrons).
- Since \(K_2Cr_2O_7\) is causing the reduction of chromium, it is acting as an oxidizing agent.

### Step 4: Identify the Role of HCl
- In this reaction, hydrochloric acid (HCl) provides chloride ions (Cl⁻) which are oxidized to chlorine gas (Cl₂).
- Thus, HCl is losing electrons and is acting as a reducing agent.

### Step 5: Evaluate the Statements
1. **\(K_2Cr_2O_7\) acts as an oxidizing agent.**
- **Correct** (as it is reduced).

2. **HCl is the reducing agent.**
- **Correct** (as it is oxidized).

3. **\(K_2Cr_2O_7\) is the reducing agent.**
- **Incorrect** (it is the oxidizing agent).

4. **HCl is the oxidizing agent.**
- **Incorrect** (it is the reducing agent).

### Conclusion
The correct statements are:
- Statement 1: Correct
- Statement 2: Correct
- Statement 3: Incorrect
- Statement 4: Incorrect

### Final Answer
The correct statements are 1 and 2.

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