Hydrogen sulfide, H2S, is a foul-smelling gas. It burns to form sulfur dioxide.

Question

2H2S9(g) + 3O2(g) → 2SO2(g) + 2H2O(g); ∆H = -1037kJ
Calculate the enthalpy change to burn 36.9g of hydrogen sulfide

Answer 1

I corrected a typo where you typed a 9 before the (.
2H2S(g) + 3O2(g) → 2SO2(g) + 2H2O(g) ∆H = -1037kJ
Calculate the enthalpy change to burn 36.9g of hydrogen sulfide

So dH is -1037 kJ for 2*(2 + 32) = 2*34 = 68 g H2S. Easy to convert to 36.9 g this way. -1037 kJ x ((36.9/68) = ? OR you can set up a proportion like this.
(-1037 kJ/68 g) = (x kJ/36.9 g) and solve for x