Final answer:
The given equation is false as it is not properly balanced to represent a redox reaction, where an oxidation and a reduction must occur through the transfer of electrons, reflected in a change in oxidation states.
Step-by-step explanation:
The equation 2Cr + 3Cl2 → 2CrCl3 should be 2Cr + 3Cl2 → 2CrCl3 to properly represent a redox reaction, where chromium is oxidized and chlorine is reduced. In a redox reaction, there must be an exchange of electrons, with one species being oxidized (losing electrons) and another being reduced (gaining electrons). The incorrect formula 2CrCl suggests an imbalance in charges, which does not align with the conservation of charge principle. Therefore, the given equation is false because it is not properly balanced to reflect the changes in oxidation states that occur during a redox reaction.