The molecular formula for the compound is [tex]C_{4} H_{8}[/tex] .
% of C = 79.85%
% of H = 20.15%
Let the mass of the compound be 100g, then
Mass of C = 70.85 g
Mass of H = 20.15 g
Molar mass = 60.15 g/mol
Moles of Carbon = [tex]\frac{79.85}{12.01 g/mol}[/tex]
= [tex]6.64 mol[/tex]
Moles of Hydrogen = [tex]\frac{20.15}{1.00794 g/mol}[/tex]
= [tex]19.99 mol[/tex]
And we divide both sides by the lower quantity;
[tex]C_{\frac{6.64 mol}{6.64 mol} } H_{\frac{19.99 mol}{6.64 mol} }[/tex] ≅ CH₂
And [tex](empirical formula)_{n} = molecular formula[/tex]
60.15 g/mol = n × ( 12.01 + 2 × 1.00794)
n = 4
Therefore, the molecular formula for the compound is [tex]C_{4} H_{8}[/tex] .
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