The standard state of bromine at \(298\text{ K}\) and \(1\text{ atm}\) is \(\text{Br}_2\text{(l)}\). A student compares the standard enthalpy changes for the two reactions represented below at \(298\text{ K}\):

\[ \text{Reaction 1: } \text{H}_2\text{(g)} + \text{Br}_2\text{(l)} \rightarrow 2\text{HBr(g)} \quad \Delta H_1^\circ \]
\[ \text{Reaction 2: } \text{H}_2\text{(g)} + \text{Br}_2\text{(g)} \rightarrow 2\text{HBr(g)} \quad \Delta H_2^\circ \]

Which of the following correctly compares \(\Delta H_2^\circ\) to \(\Delta H_1^\circ\) and provides the correct justification?