When a Student Performs an Endothermic Reaction in a Calorimeter $\Delta$

When a student performs an endothermic reaction in a calorimeter, how (if any) does the calculated value of $\Delta$ H differ from the actual value if the heat exchanged with the calorimeter is not taken into account?

A) ( $\Delta$ H_calc) is less positive because the reaction absorbs heat from the calorimeter.
B) ( $\Delta$ H_calc) equals the actual value because the calorimeter does not absorb heat.
C) ( $\Delta$ H_calc) is more negative because the calorimeter always absorbs heat from the reaction.
D) ( $\Delta$ H_calc) is less negative because the calorimeter absorbs heat from the reaction.
E) ( $\Delta$ H_calc) is more positive because the reaction absorbs heat from the calorimeter.