An unknown compound that possess a molar mass of 151.2 g/mol was analyzed and fo

Question

An unknown compound that possess a molar mass of 151.2 g/mol was analyzed and found to be composed of 53.3% oxygen, 6.7% hydrogen and 40.0% carbon. What is the empirical formula of this compound? Given the stated molar mass, what is the molecular formula of the compound? What is the molarity of a solution that is prepared by placing 3.97 grams of sodium carbonate, Na_2CO_3 into 500mL of water? Report your answer using the correct units for molarity. For the solution that is prepared in problem 2, identify the solute, and the solvent? Solute: ____________ Solvent: ______________ Regrade Policy: If you believe your quiz has been unfairly graded you must return the quiz to the TA before you leave the discussion room. He/She will get the quiz to me and I will regrade it completely. You should be aware that if you elect to do this, your grade may be higher, the same, or lower, depending on whether or not other problems were graded correctly.

Explanation / Answer

Mol ratio of O :H : C = (53.3/16) : (6.7/2) : (40/12) = 3.33 : 6.7 : 3.33 = 1:2:1

Emperical formula = (CH2O)x

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12x + 2x + 16x = 151.2

or, x = 5.04 ~5

Molecular formula = C5H10O5

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