Believe this to be Carbon hydroxide
The empirical formula C2OH4 simplifies to C1O2H2. To find the molecular formula, divide the molar mass (88 g/mol) by the empirical formula mass (112 + 216 + 2*1 = 46 g/mol) to get 1.91. This means the molecular formula is approximately 1.91 times the empirical formula, so the molecular formula is C2O4H4.
Look at your atomic masses for phosphorus and oxygen. Set up 2.5/31 and 3.23/16. This makes 0.08 and 0.2. Now consider 0.08/0.2 to equal 0.4. So, your ratio of P to O is 0.4, which is 4/10. So, your formula, which reflects that ratio, is P4O10. That's tetraphosphorus decoxide, a molecular solid used in match-heads.