CHEMISTRY COMMUNITY

Can someone explain the transfer of energy that happens when both delta H and w are negative and positive?

I know the when work is positive, energy is going into the system. This means that some sort of pressure is condensing the system or the volume is getting smaller.

When delta H is negative, is heat flowing into the system or leaving the system?

A negative Delt. H means a -q (heat loss)

A negative delta H means that the heat transfer is negative and thus the system is losing heat.

-delta H means the system is exothermic and is releasing heat (surrounding absorb that heat) and + delta H means the system is endothermic and requires heat

w>0 means work is being done on the system
w<0 means work is being done by the system
H>0 means the system requires heat (heat flows in)
H<0 means the system release heat (heat flows out)

The sign of enthalpy is determined with respect to the system. Therefore, when ΔH is negative, you know heat is decreasing with respect to the system. This is the conventional way of writing signs unless otherwise stated.

Work greater than 0 means work is done on the system; work less than 0 means that work is done on the surroundings. deltaH greater than 0 means heat is flowing in the system and deltaH less than 0 means that heat is flowing out of the system (assuming constant pressure).