Empirical formula help¬̐̑ͦ̅͏̸̵̡̪͎̼̖̬̝̘͍̭͎̪̖̮͈̘͠ ͪ̓̚¬̧̡͚͖͉̩̘̰̼̦͕̣̺̰ͣ͂̅̒͗͑̎̐͊̿̏͋́̚ͅ ̈́ͨ͒ͧ̂̿̇̉ͪ̊̚͏̸̜̭̱͓͎̖

A 0.400g sample of a whit powder contains 0.414g of potassium, 0.115g of surfer, and 0.144g of oxygen. What is the empirical formula for this compound? Explain how you got your answer.
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̵̴̞̞̯͎̱̠̦̖̄ͭͤ͒ͩ͠͞ ̧̧͚̙̗̠̗̗̥̯̜͙͂̾ͩ̋̉͑͗͊ͭ̉̓̇ͦ̿͂̌͟͠ȼ̇ſ̵̴̞̞̯͎̱… ̧̧͚̙̗̠̗̗̥̯̜͙͂̾ͩ̋̉͑͗͊ͭ̉̓̇ͦ̿͂̌͟͠ȼ̇ſ̵̴̞̞̯͎̱… ̧̧͚̙̗̠̗̗̥̯̜͙͂̾ͩ̋̉͑͗͊ͭ̉̓̇ͦ̿͂̌͟͠ȼ̇ſ̵̴̞̞̯͎̱… ͚̙̗̠̗͂̾ͩ

mass of K = .141 g ; moles of K = .141 / 39 = 0.00362 moles

mass of sulfur = .115g = .115 / 32 moles = 0.003594

mass of O = .144 g = .144 / 16 moles of O = 0.0090

molar ratio of K : S : O = 0.00362 : 0.003595: 0.0090

dividing by the smallest number we simplify the ratio to get

1.0: 1.0: 2.5 to get whole numbers we x 2

and get 2:2:5

empirical formula is K2S2O5

well, and here's the tricky part, you have a white powder containing 0.673g of elements and the sample is only 0.4g in mass. do you see a problem here?