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A 0.507-g sample of a compound containing only carbon, hydrogen and oxygen is burned in oxygen gas to produce 0.698 g of CO2 and 0.571 g of H2O. A member of your study group solves this problem by finding that the CO2 and H2O together contain 0.190 g C, 0.0639 g H, and 1.015 g O; this gives a mole ratio of 1:4:4 and a formula of CH4O4. What conceptual error did he make? Determine the correct empirical formula for this compound.

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Category:- Chemistry
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