Reactions do not just make product — they move heat, and they move it by the mole: $q = n\,\Delta H$ — read aloud: q equals n delta-H. $\Delta$ is the Greek capital delta (delta, chemistry's “change in”), and $\Delta H$ is the molar enthalpy change: the heat fare each mole pays, in kJ/mol. The units run the whole show — $\mathrm{mol} \times \mathrm{kJ/mol} = \mathrm{kJ}$, the mole cancels, pure heat remains.

The SIGN of $\Delta H$ is a direction, not a difficulty: negative means the heat leaves (exothermic — burning, hand warmers), positive means the heat is absorbed (endothermic — cold packs). At this rung the words in the question already say which way the heat flows, so compute with magnitudes and let “released” or “absorbed” speak the sign. It gets trapped later; here it just gets taught.