Delta E and Delta H relationship question

CH_3_OH (g) +H_2_ ------> CH_4_(g)+ H_2_O (g)
Delta H = -115.4 kJ
Delta G = -117.3 kJ

True/False
Delta E and Delta H for the reaction are approximately equal?

What is the state for H2? If it is gaseous, then I would say H and E are approximately equal because there is no pressure-volume work being done in the question.

CH3OH(g) + H2(g) --> CH4(g) + H2O(g)
change in gaseous moles = gaseous moles of product - gaseous moles of reactant
change in gaseous moles = 2 mol - 2 mol = 0

Pressure-volume work = -PV = -nRT = -(0 * 8.314J/molK * 298K)

delta E (internal energy) = H + W
delta E = -115.4kJ + 0
delta E = -115.4kJ