Which of the following statements is/are correct?

Options

A. Chloropicrin `(C Cl_(3).NO_(2))` can made cheapy for use as an insectide by the following reaction:
`CH_(3) NO_(2) + Cl_(2) rarr C Cl_(3) NO_(2) + HCl`
B. In a rocket motor fueled with butane `(C_(4) H_(10))`, 0.1 mol of butane requires `14.56 L` of `O_(2)` at `STP` for complete combustion.
C. A portable hydrogen generator utilises the reaction:
`(CaH_(2) + H_(2)O rarr Ca (OH)_(2) + H_(2)), 2.1 g "of" CaH_(2)` would produce `2.24 L` "of" `H_(2)` at `STP`
D. In the Mond process for purifying nickel, the volatile nickel carbonyl `[Ni(CO)_(4)]` is produced by the reaction. `Ni + Co rarr Ni (CO)_(4). 58.8 7g` of `Ni` utilises `89.6 L` of `CO` at standard conditions.

Explanation

To determine which of the statements regarding chloropicrin, butane combustion, hydrogen generation, and the Mons process for nickel purification are correct, we will analyze each statement step by step.

### Step 1: Analyze Statement A
**Statement A:** "Chloropicrin can be made cheaply for use as an insecticide by the following reaction."

1. **Identify the reactants:** The reaction involves CH3NO2 and Cl2.
2. **Determine the mechanism:** The reaction is expected to proceed via a free radical mechanism.
3. **Assess the stability of the free radical:** The free radical formed from CH3NO2 is unstable due to the -I (inductive) effect of the nitro group (NO2), which increases positive charge density on the carbon, making the radical less stable.
4. **Conclusion:** Since the free radical is unstable, chloropicrin cannot be formed from this reaction. Thus, **Statement A is false.**

### Step 2: Analyze Statement B
**Statement B:** "In a rocket motor fuel with butane, 0.1 mole of butane requires 14.56 moles of O2 at Hgp for complete combustion."

1. **Write the balanced equation for combustion of butane (C4H10):**
\[ C_4H_{10} + O_2 \rightarrow CO_2 + H_2O \]
2. **Balance the equation:**
- Carbon: 4 CO2
- Hydrogen: 5 H2O
- Total O2 needed: 4 (from CO2) + 5/2 (from H2O) = 13/2
3. **Calculate O2 required for 0.1 mole of butane:**
\[ O_2 = 0.1 \times \frac{13}{2} = 0.65 \text{ moles} \]
4. **Convert moles of O2 to liters at STP:**
\[ \text{Volume of } O_2 = 0.65 \times 22.4 \text{ L} = 14.56 \text{ L} \]
5. **Conclusion:** **Statement B is correct.**

### Step 3: Analyze Statement C
**Statement C:** "A portable hydrogen generator utilizes the reaction of calcium hydride (CaH2) with water."

1. **Write the balanced reaction:**
\[ CaH_2 + 2H_2O \rightarrow Ca(OH)_2 + H_2 \]
2. **Determine moles of CaH2 from given mass (2.1 g):**
- Molar mass of CaH2 = 42 g/mol
\[ \text{Moles of } CaH_2 = \frac{2.1}{42} = 0.05 \text{ moles} \]
3. **Calculate moles of H2 produced:**
\[ \text{Moles of } H_2 = 2 \times 0.05 = 0.1 \text{ moles} \]
4. **Convert moles of H2 to volume at STP:**
\[ \text{Volume of } H_2 = 0.1 \times 22.4 \text{ L} = 2.24 \text{ L} \]
5. **Conclusion:** **Statement C is correct.**

### Step 4: Analyze Statement D
**Statement D:** "In the Mons process for purifying nickel, 58.587 grams of nickel utilizes 89.96 grams of carbon monoxide."

1. **Write the reaction for the Mons process:**
\[ Ni + 4CO \rightarrow Ni(CO)_4 \]
2. **Calculate moles of nickel:**
- Molar mass of Ni = 58.69 g/mol
\[ \text{Moles of Ni} = \frac{58.587}{58.69} \approx 1 \text{ mole} \]
3. **Determine moles of CO required:**
\[ \text{Moles of CO} = 4 \times 1 = 4 \text{ moles} \]
4. **Convert moles of CO to grams:**
- Molar mass of CO = 28 g/mol
\[ \text{Mass of CO} = 4 \times 28 = 112 \text{ g} \]
5. **Conclusion:** The statement claims 89.96 g is required, which is incorrect. **Statement D is false.**

### Final Conclusion
- **Correct Statements:** B and C
- **Incorrect Statements:** A and D

### Summary of Correctness
- **A:** Incorrect
- **B:** Correct
- **C:** Correct
- **D:** Incorrect