When 1000 Moles of H₂(g)reacts with 5

When 10.00 moles of H₂(g) reacts with 5.000 mol of O₂(g) to form 10.00 mol of H₂O(l) at 25°C and a constant pressure of 1.00 atm.If 683.0 kJ of heat are released during this reaction,and PΔV is equal to - 37.00 kJ,then

A) ΔH° = + 683.0 kJ and ΔE° = + 720.0 kJ.
B) ΔH° = + 683.0 kJ and ΔE° = + 646.0 kJ.
C) ΔH° = - 683.0 kJ and ΔE° = - 646.0 kJ.
D) ΔH° = - 683.0 kJ and ΔE° = - 720.0 kJ.