Answer to Question #98351 in General Chemistry for Spencer
2019-11-09T23:58:36-05:00
A sample of an unknown compound, composed only of carbon and hydrogen, produced 2.56g of CO2 and 0.786g of H2O in a combustion analysis. What is the empirical formula of the unknown compound?
1
2019-11-11T07:47:43-0500
Find moles of C:
"n(C) = n(CO_2)= \\frac{m}{M} = \\frac{2.56}{44.01} = 0.0582 mol" Find moles of H
"n(H) = 2\\times n(H_2O) = 2\\times \\frac {m(H_2O)}{M(H2O)} = 2\\times \\frac{0.786}{18.02} = 0.0872 mol" Find ratio n(C):n(H)
"n(C):n(H) = 0.0582:0.0872 = \\frac{0.0582}{0.0582}:\\frac{0.0872}{0.0582} = 1: 1.5 = 2:3" Empirical formula is
"C_2H_3"
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