consider +1 and +2 oxidation states for metals 
case 1 :
M2O + H2  -- > 2M  +H2O
2x+16                 2x
so, its , 2*3.15/(2x+16) = 1.05/x 
 or x= 4 i.e., the compound may be Helium(but helium being inert gas doesn't for oxide)
case 2 :
MO + H2  -- > M  +H2O
x+16                 x
so, its , 3.15/(x+16) = 1.05/x 
 or x = 8 (but there is no element with atomic weight of 8)
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actually it can be much more easier . we all know that there is no metal with atomic mass of 8 and helium doesn’t form oxide . so the answer can be calculated by the following method:
mass of metal/massof oxygen(both given in ques.)= eq. mass of metal (E) /eq.mass of oxygen (i.e.8)
1.05 / (3.15-1.05) =E/8
E=4
 
						

							Simply apply the relationship between equivalent wt. And mass of element i.e.Mass of element/eq.of element=mass of oxid