ld 145412748&0penVellumHMAC-a899daa13726d317502bbdfd422dcace 10001 HW 44-Google

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ld 145412748&0penVellumHMAC-a899daa13726d317502bbdfd422dcace 10001 HW 44-Google Chrome Secure https//session masteringchemistry.com/myct/itemViewlassignmentProblemID-100266312&offset-next; Exercise 3.98 Constants l Periodic Table Part A Tartaric acid is the white, powdery substance that coats sour candies such as Sour Patch Kids Combustion analysis of a 1201-g sample of tartaric acid-which contains only carbon, hydrogen, and oxygen-produced 14.08 g CO and 4.32 gH2O Find the empirical formula for tartaric acid Express your answer as a chemical formula. Sutbimit Provide Feedback

Explanation / Answer

All the Carbon in Hydrocarbon will completly converted to CO2
So the number of moles of CO2 = mass of CO2 / Molar mass of CO2
= 14.08 g / 44 (g/mol )
= 0.32 mol
Each CO2 has 1 mole of C in it, therefore the number of moles of C = moles CO2 = 0.32 mol

Mass of C= number of moles x molar mass= 0.32 mol x 12 g/ mol = 3.84 g
All the Hydrogen present in the given hydrocarbon will ends up into H2O
So the number of moles of H2O = mass of H2O / Molar mass of H2O
= 4.32 g / 18(g/mol)
= 0.24 mol
Each H2O has 2 H atoms, so number of moles of H = 2 x number of moles of H2O = 2x0.24= 0.48 mol

Mass of H = number of moles x molar mass= 0.48*1= 0.48 g

Mass of O = mass of tartaric acid -( mass of O + mass of H)

= 12.01-(3.84+0.48)= 7.69 g

Number of moles of O= mass / molar mass= 7.69 g/ 16(g/ mol)= 0.48 mol
The ratio of moles O C to H to O is = 0.32: 0.48:0.48
Divide each number in the ratio by the smallest number we get C:H:O= 1: 1.5 : 1.5 . OR. 2:3:3
Therefore the emperical formula is C2H3O3

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