1. The problem statement, all variables and given/known data Complete combustion of a 0.0150 mol sample of a hydrocarbon, CxHy, gives 1.680L of CO2 at STP and 0.810g of H2O a) what is the molecular formula b) what is empirical formula 2. Relevant equations pv=nRt 3. The attempt at a solution a) mol of co2: n=pv/Rt=1 atm * 1.680L/0.0821*273= 0.074955495mol - Mol of h2o: 0.810g/18.02g/mol * 2 = 0.08990011 mol H2 mol ratio: 0.08990011/0.074955495= 1.199379845... * 5 = 6 molecular formula: c5h6. Is this wrong? is it possible to multiply by four and round the number to 5 instead of 6? so that it would be c4h5? Or is the above one correct? also: how do i get the molecular formula? i cant get a lowest whole number ratio here. Thanks!