The heat content of the products is more than that of the reactant in an ............. reaction.
In this question the answer given is "exothermic"; yet I thought the answer would be endothermic as the products have more heat content and energy cannot be created nor destroyed. Therefore, from the reactants' side, more energy should have been put in for the heat content of the products to be greater.
Also mathematically endothermic make sense as: $$\Delta_\mathrm{r}H = \sum \Delta_\mathrm{f}H_\mathrm{P}-\sum \Delta_\mathrm{f}H_\mathrm{R}$$
And as: $\sum \Delta_\mathrm{f}H_\mathrm{P} \gt \sum \Delta_\mathrm{f}H_\mathrm{R}$ ,$\Delta_\mathrm{r}H \gt 0$
Could someone please explain where am I wrong and why the answer is 'exothermic'?