Chromyl chloride test side products
If you write the ionic equation, it seems that chlorine gas will produce. However, we see their half equation and standard potential.

$$\ce{ Cr2O7^2- + 14H+  + 6e-  -&gt;  2Cr^3+  + 7H2O}$$
Standard potential: $E^\circ = \pu{+1.33V}$

$$\ce{ 6Cl-  -&gt;  3Cl2 + 6e-}$$
Standard potential: $E^\circ = \pu{-1.36V}$

Thus, the standard potential cell for this ionic you say is equal to  $$\pu{+1.33V} + (\pu{-1.36V}) = \pu{-0.03V}$$

Because the standard potential cell is negative, so, it is call not energetically feasible or this reaction will not happen.

P.S.: The explanation only work under standard conditions.