28. 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)\( \Delta H_{\text{calc}} \) is more negative because the calorimeter always absorbs heat from the reaction.
(B)\( \Delta H_{\text{calc}} \) is less negative because the calorimeter absorbs heat from the reaction.
(C)\( \Delta H_{\text{calc}} \) is more positive because the reaction absorbs heat from the calorimeter.
(D)\( \Delta H_{\text{calc}} \) is less positive because the reaction absorbs heat from the calorimeter.
(E)\( \Delta H_{\text{calc}} \) equals the actual value because the calorimeter does not absorb heat.