How many of the following have zero dipole moment? $\begin{array}{l}{\mathrm{CCl}}_{4,}{\mathrm{C}}_2{\mathrm{O}}_3,{\mathrm{C}}_3{\mathrm{O}}_2,\mathrm{CO},{\mathrm{CS}}_2,{\mathrm{CO}}_2,:{\mathrm{CCl}}_2,{\mathrm{CH}}_2{\mathrm{Cl}}_2,\\ {\mathrm{C}}_2{\mathrm{H}}_2\end{array}$

Even though $\mathrm{C}$ and $\mathrm{Cl}$  have different electronegativities and each $\mathrm{C} - \mathrm{Cl}$bond is polar and has some dipole moment, the carbon tetrachloride molecule has zero dipole moment.
Tricarbon dioxide, often known as carbon suboxide, has the chemical formula ${\mathrm{C}}_3{\mathrm{O}}_2$ o or  $\mathrm{O}=\mathrm{C}=\mathrm{C}=\mathrm{C}=\mathrm{O}$. It is a cumulene because of its four double bonds in total.
While ${\mathrm{H}}_2\mathrm{O} \left({\mathrm{SO}}_2\right)$has some dipole moment, ${\mathrm{CO}}_2 \left({\mathrm{CS}}_2\right)$ has no dipole moment. A polar molecule's ability to rotate or align itself in an electric field is measured by its dipole moment. A vector element is the dipole moment.
The chemical formula for ${\mathrm{CO}}_{2 }$is $\mathrm{O}=\mathrm{C}=\mathrm{O}$, and it contains a bond dipole moment ($\mathrm{C}-\mathrm{O}$ bond). However, because one bond's dipole moment is negated by another, the structure of ${\mathrm{CO}}_2$is

This is zero dipole moment are :

${\mathrm{CCl}}_4, {\mathrm{C}}_3{\mathrm{O}}_2,{ \mathrm{CS}}_2,{ \mathrm{CO}}_2, {\mathrm{C}}_2{\mathrm{H}}_2$