Follow up question: Explain why the reaction of aluminum metal with aqueous sulfuric acid solution has very nearly the same ΔH value as the reaction between aluminum metal and HCl? Consider the atomic level.
All I have is that they have the same net ionic equations. The total energy absorbed in bonding break is similar in each equation due to this, which is less energy than in bond making. This makes both exothermic close in values. (Does the fact that they are both strong acids have anything to do with this?)
P.S. Thanks for all the help! This site is really clarifying my understanding:)