If a Student Performs an Endothermic Reaction in a Calorimeter,how $\Delta$

If a student performs an endothermic reaction in a calorimeter,how 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" would be more negative because the calorimeter always absorbs heat from the reaction.
B) " $\Delta$ H_calc" would be less negative because the calorimeter would absorb heat from the reaction.
C) " $\Delta$ H_calc' would be more positive because the reaction absorbs heat from the calorimeter.
D) " $\Delta$ H_calc" would be less positive because the reaction absorbs heat from the calorimeter.
E) " $\Delta$ H_calc" would equal the actual value because the calorimeter does not absorb heat.