A 4.043 sample of a compound containing only carbon, hydrogen, and oxygen is burned in an excess of dioxygen, producing 9.191 g CO2 and 3.762 g H2O.

A 4.043 sample of a compound containing only carbon, hydrogen, and oxygen is burned in an excess of dioxygen, producing 9.191 g CO2 and 3.762 g H2O. What percent by mass of oxygen is contained in the original sample? show your work and explain.

Expert Solution

moles of CO2 = mass / molar mass

= 9.191 / 44

= 0.2089

mass of C = 0.2089 x 12 = 2.507 g

moles of H2O = 3.762 / 18 = 0.209

moles of H = 2 x 0.209 = 0.418

mass of H = 0.418

mass of O = total mass - (mass of C + mass of H )

= 4.043 - (2.507 + 0.418)

= 1.118 g

percent by mass of oxygen = ( mass of O / total mass ) x 100

= (1.118 / 4.043 ) x 100

= 27.65 %

queen_honey_blossom answered 2 years ago

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