Complete combustion of 7.50 g of a hydrocarbon produced 23.1 g of co2 and 10.6 g of h2o. what is the empirical formula for the hydrocarbon ?

Chemical reaction: CₓHₐ + O₂ → xCO₂ + a/2H₂O.
m(CₓHₐ) = 7,50 g.
m(CO₂) = 23,1 g.
m(H₂O) = 10,6 g.
n(CO₂) = m(CO₂) ÷ M(CO₂).
n(CO₂) = 23,1 g ÷ 44 g/mol.
n(CO₂) = n(C) = 0,525 mol.
n(H₂O) = 10,6 g ÷ 18 g/mol = 0,588.
n(H₂O) : n(H) = 1 : 2.
n(H) = 1,176 mol.
n(H) : n(C) = 1,176 mol : 0,525 mol.
n(H) : n(C) = 2,25 : 1 /×4.
n(H) : n(C) = 9 : 4.
C₄H₉.

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