Total number of compound among the followinng having zero dipolemoment is/are `C Cl_(4),CH_(3)Cl,CH_(2)Cl_(2),CHCl_(3)`, o-, m-and p-dichlorobenzene, benzyl chloride, benzal dichloride, benzotrichloride.

Explanation

To determine the total number of compounds among the given list that have a zero dipole moment, we need to analyze each compound based on its molecular geometry and symmetry. A molecule has a zero dipole moment if the individual bond dipoles cancel each other out due to symmetry.

### Step-by-Step Solution:

1. **Identify the Compounds:**
The compounds given are:
- CCl₄ (Carbon Tetrachloride)
- CH₃Cl (Methyl Chloride)
- CH₂Cl₂ (Methylene Chloride)
- CHCl₃ (Chloroform)
- o-Dichlorobenzene
- m-Dichlorobenzene
- p-Dichlorobenzene
- Benzyl Chloride
- Benzal Dichloride
- Benzotrichloride

2. **Analyze CCl₄:**
- **Geometry:** Tetrahedral
- **Symmetry:** The four Cl atoms are symmetrically arranged around the central C atom.
- **Dipole Moment:** The dipoles cancel out.
- **Conclusion:** CCl₄ has a zero dipole moment.

3. **Analyze CH₃Cl:**
- **Geometry:** Tetrahedral
- **Symmetry:** Asymmetrical due to one Cl atom and three H atoms.
- **Dipole Moment:** The dipole does not cancel out.
- **Conclusion:** CH₃Cl does not have a zero dipole moment.

4. **Analyze CH₂Cl₂:**
- **Geometry:** Tetrahedral
- **Symmetry:** Asymmetrical due to two Cl atoms and two H atoms.
- **Dipole Moment:** The dipoles do not cancel out.
- **Conclusion:** CH₂Cl₂ does not have a zero dipole moment.

5. **Analyze CHCl₃:**
- **Geometry:** Tetrahedral
- **Symmetry:** Asymmetrical due to three Cl atoms and one H atom.
- **Dipole Moment:** The dipoles do not cancel out.
- **Conclusion:** CHCl₃ does not have a zero dipole moment.

6. **Analyze o-Dichlorobenzene:**
- **Geometry:** Planar
- **Symmetry:** Asymmetrical due to the position of the Cl atoms.
- **Dipole Moment:** The dipoles do not cancel out.
- **Conclusion:** o-Dichlorobenzene does not have a zero dipole moment.

7. **Analyze m-Dichlorobenzene:**
- **Geometry:** Planar
- **Symmetry:** Asymmetrical due to the position of the Cl atoms.
- **Dipole Moment:** The dipoles do not cancel out.
- **Conclusion:** m-Dichlorobenzene does not have a zero dipole moment.

8. **Analyze p-Dichlorobenzene:**
- **Geometry:** Planar
- **Symmetry:** Symmetrical due to the two Cl atoms being opposite each other.
- **Dipole Moment:** The dipoles cancel out.
- **Conclusion:** p-Dichlorobenzene has a zero dipole moment.

9. **Analyze Benzyl Chloride:**
- **Geometry:** Planar
- **Symmetry:** Asymmetrical due to the presence of one Cl atom.
- **Dipole Moment:** The dipole does not cancel out.
- **Conclusion:** Benzyl Chloride does not have a zero dipole moment.

10. **Analyze Benzal Dichloride:**
- **Geometry:** Planar
- **Symmetry:** Asymmetrical due to the presence of two Cl atoms.
- **Dipole Moment:** The dipoles do not cancel out.
- **Conclusion:** Benzal Dichloride does not have a zero dipole moment.

11. **Analyze Benzotrichloride:**
- **Geometry:** Planar
- **Symmetry:** Asymmetrical due to the presence of three Cl atoms.
- **Dipole Moment:** The dipoles do not cancel out.
- **Conclusion:** Benzotrichloride does not have a zero dipole moment.

### Final Count:
The compounds with zero dipole moments are:
- CCl₄
- p-Dichlorobenzene

**Total Compounds with Zero Dipole Moment: 2**