Which alkene reacts faster with HCl?
This is an exercise in applying the Hammond postulate (multiple times). To accurately compare reaction rates, we need to have the activation energy. We don't have this, and the actual energy of the transition state is unknowable without experimental data.
Hammond's postulate states that the structure of the transition state is more similar  to the intermediate to which it is closer in energy. For these reactions, the formation of the carbocation is endergonic, so the transition states look more like the carbocation than the alkene. We can then make some assumptions about the relative energies of the transition states from the energy change of the mechanism step if some things remain the same.
For example, alkene 3 can be protonated to form two different carbocations: A and B.

Using PM6 calculations in MOPAC, I calculated the heats of formation of alkene 3 and cations A and B.
$$\begin{array}{l|r} 
&amp; \mathrm{\Delta_r H^\circ \ (kJ/mol)} \\ \hline 
3 &amp; -42.1 \\
\mathrm{A} &amp; 710.7 \\
\mathrm{B} &amp; 702.6\\
\end{array}$$
Since we are starting from the same place (alkene 3), we can postulate that cation B forms more quickly than cation A because it is slightly lower in energy.
You need to do similar analysis for all your alkenes and the cations they can form. In some cases you have two alkenes that might form the same cation. In that case, the higher energy alkene would likely translate into the more rapid reaction.
You do not need to go and calculate all the energies. You should have learned some rules by now to assess the relative stability of alkenes and carbocations based on substitution pattern.