Rate of EAS in chlorobenzene and fluorobenzene
We need some data to answer your question. As presented in this earlier answer (which is also relevant to this question), here are the relative rates for electrophilic aromatic nitration of the halobenzenes compared to benzene itself.

\begin{array}{|c|c|c|c|} \hline
\ce{Ar-X} &amp; \text{Relative Rate}  \\ 
\hline
\ce{Ar-H} &amp; 1.0 \\ \hline
\ce{Ar-F} &amp; 0.11 \\ \hline
\ce{Ar-Cl} &amp; 0.02 \\ \hline
\ce{Ar-Br} &amp; 0.06  \\ \hline
\ce{Ar-I} &amp; 0.13 \\ \hline
\end{array}

You are correct that inductive and resonance effects operate in opposite directions here. All of the halogens are more electronegative than hydrogen so they inductively remove electron density from the aromatic ring and tend to slow the reaction down. Whereas resonance effects would donate electron density into the aromatic ring and speed the reaction up.

However it is not correct to say 


  On comparison of resonance effect and inductive effect, resonance
  effect dominates over inductive effect


Here is a series where inductive effects play a larger role than resonance effects.  This is why all of the halobenzenes react more slowly than benzene itself.

In fluorobenzene the overlap between carbon 2p and fluorine 2p orbitals is very effective, but the carbon 2p orbital cannot overlap as effectively with higher p orbitals (e.g. chlorine 3p, bromine 4p, etc.). It is the stronger resonance contribution from this effective electron donating resonance interaction with fluorine that makes fluorobenzene more reactive towards electrophilic aromatic substitution than chlorobenzene.

The electrophilic reactivity of the other halobenzenes is also controlled by a blend of resonance and inductive effects.  As we move down the series from chlorine to iodine the electronegativity decreases and the strength of the electron withdrawing inductive effect also decreases - this should speed up the rate of reaction. However the strength of the resonance effect also decreases due to less effective orbital overlap between halogen and carbon - this should slow the reaction down. Looking at the data we can see that the reaction rate slowly increases as we move from chlorine to iodine, suggesting that the inductive effect is still the primary effect with resonance, as expected due to poorer overlap, still playing a secondary role.