How many grams of oxygen gas are required to produce 7.46 kJ of heat when hydrogen gas burns at constant pressure to produce gaseous water?

Question

2 H2(g) + O2(g) → 2 H2O(g) ΔH = −484 kJ
Liquid water has a heat of vaporization of 44.0 kJ per mole at 25°C.

Answer 1

484 kJ heat released from 4 g hydrogen.
44.0 kJ heat used to vaporize the water/mole or 88 kJ heat used to vaporize 4 g hydrogen.
484-88 = 396 kJ net heat released.
So We need 484 x (x grams/4) = 7.46 g hydrogen burned to produce the 396 kJ.
Solve for x THEN CHECK IT TO MAKE SURE THE REACTION RELEASES ENOUGH TO USE UP THE AMOUNT NEEDED TO VAPORIZE AND LEAVE YOU WITH 7.45 kJ.
Check my thinking.