Use the table to answer the question reaction CH4 + cl2 ccl4 + 4 HCL which statement about the change in the bond energy of this reaction is correct
Without the table, I cannot provide specific information about the change in bond energies for the given reaction. However, if we assume that CH4 is methane, Cl2 is chlorine gas, CCl4 is carbon tetrachloride, and HCl is hydrogen chloride, we can make a general statement about the change in bond energy based on the reaction equation:
In the given reaction, CH4 (methane) and Cl2 (chlorine gas) react to form CCl4 (carbon tetrachloride) and 4 HCl (hydrogen chloride).
To form the products, the bonds in the reactants must be broken, and new bonds in the products are formed. In this case, the methane molecule's four C-H bonds and the chlorine gas's Cl-Cl bond are broken. Meanwhile, carbon tetrachloride forms four C-Cl bonds, and hydrogen chloride forms four H-Cl bonds.
Since the bonds in the reactants are being broken and new bonds are being formed in the products, it can generally be inferred that the overall change in bond energy for this reaction is endothermic (requires energy input). This is because energy is needed to break the existing bonds, and less energy is released when new bonds are formed.
However, to accurately determine the change in bond energy, the table would be required to provide the specific bond energies involved in the reaction.